Chemistry Exam 2024: The Chemical Awakens
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Questions and Answers

What are the products formed in a neutralisation reaction between an acid and a base?

  • Salt and hydrogen gas
  • Water and carbon dioxide
  • Salt and water (correct)
  • Salt and oxygen

What occurs during a redox reaction?

  • Only one reactant undergoes reaction
  • Both reactants are oxidised
  • One reactant is reduced and the other is oxidised (correct)
  • No change occurs in the oxidation states

What type of reaction is characterized by the combination of oxygen with a compound to produce carbon dioxide and water?

  • Decomposition
  • Double displacement
  • Neutralisation
  • Combustion (correct)

What indicates a reversible reaction in a chemical equation?

<p>A double arrow (B)</p> Signup and view all the answers

How does the atomic radius change as you move down a group in the periodic table?

<p>It increases (D)</p> Signup and view all the answers

What trend in electronegativity is observed across a period from left to right?

<p>It increases (C)</p> Signup and view all the answers

Which statement about valence electrons in the periodic table is correct?

<p>Elements in the same group have the same number of valence electrons (A)</p> Signup and view all the answers

What happens to the atomic radius as you move across a period from left to right?

<p>It decreases (C)</p> Signup and view all the answers

How does the atomic radius affect the ease of ionization as you move down a group?

<p>It becomes easier to remove electrons as they are further from the nucleus. (D)</p> Signup and view all the answers

Which of the following properties decreases down Group VII elements?

<p>Electronegativity (D)</p> Signup and view all the answers

What type of compounds do Group VII elements usually form when reacting with metals?

<p>Ionic compounds (D)</p> Signup and view all the answers

Which of the following statements about Period 3 elements is true?

<p>They are good conductors of heat and electricity. (A)</p> Signup and view all the answers

What happens to the ability of Group VII elements to share electrons as you move down the group?

<p>Their ability to share electrons decreases. (A)</p> Signup and view all the answers

How do Period 3 elements primarily exist at room temperature?

<p>Primarily solids except for bromine. (D)</p> Signup and view all the answers

What characteristic differentiates nonmetals generally from metals in Period 3?

<p>Nonmetals are usually brittle. (D)</p> Signup and view all the answers

Which of the following trends in electronegativity is observed in Group VII?

<p>Electronegativity decreases from fluorine to iodine. (A)</p> Signup and view all the answers

What happens to the ionization energy as one moves down a group in the periodic table?

<p>Ionization energy decreases due to increased shielding effect. (A)</p> Signup and view all the answers

Which statement best describes the trend in effective nuclear charge across a period?

<p>Effective nuclear charge increases without a corresponding increase in shielding. (B)</p> Signup and view all the answers

Why are metals considered reducing agents?

<p>Because they easily lose their valence electrons. (D)</p> Signup and view all the answers

What is the reaction of magnesium with oxygen primarily characterized as?

<p>A combustion reaction. (A)</p> Signup and view all the answers

What occurs as one moves across a period in relation to ionization energy?

<p>Ionization energy increases due to increasing effective nuclear charge. (A)</p> Signup and view all the answers

How does the shielding effect contribute to the ease of losing valence electrons in metals?

<p>Inner-shell electrons shield outer electrons, resulting in weaker attraction. (C)</p> Signup and view all the answers

Which element from Group II is most reactive when combined with other elements?

<p>Radium (A)</p> Signup and view all the answers

What is the primary factor affecting ionization energy across a period?

<p>Increased effective nuclear charge. (A)</p> Signup and view all the answers

What type of bond is formed when non-metal atoms share valence electrons?

<p>Covalent bond (A)</p> Signup and view all the answers

Lone pairs are involved in the bonding process between atoms.

<p>False (B)</p> Signup and view all the answers

Which type of bond is characterized by a force of attraction between ions of opposite charges?

<p>Ionic bond</p> Signup and view all the answers

Fluorine has _____ lone pairs of electrons.

<p>3</p> Signup and view all the answers

Which of the following correctly describes covalent bonding?

<p>Sharing of valence electrons between non-metals (D)</p> Signup and view all the answers

Match the following concepts with their correct descriptions:

<p>Ionic Bond = Formation due to electrostatic attraction between oppositely charged ions Covalent Bond = Formation by sharing of valence electrons between non-metal atoms Lone Pair = Non-bonding pair of electrons present in an atom Metal = Element that tends to lose electrons in chemical reactions</p> Signup and view all the answers

Covalent bonds can be formed between two atoms of different elements.

<p>True (A)</p> Signup and view all the answers

Which of the following statements regarding ionisation energy is correct?

<p>Ionisation energy increases as you move down a group. (D)</p> Signup and view all the answers

Effective nuclear charge is the net positive charge experienced by an electron from the nucleus.

<p>True (A)</p> Signup and view all the answers

What is the effect of increasing distance of valence electrons from the nucleus on ionisation energy?

<p>It decreases the ionisation energy.</p> Signup and view all the answers

The 1st ionisation energy refers to the energy needed to remove the _____ valence electron from a neutral atom.

<p>outermost</p> Signup and view all the answers

Match the factors affecting ionisation energy with their descriptions:

<p>Distance of valence electrons = Increased distance means less attraction Effective nuclear charge = Stronger attraction due to more protons Shielding effect = Inner electrons reduce the pull on outer electrons</p> Signup and view all the answers

What is formed as a result of a neutralisation reaction?

<p>Salt and water (B)</p> Signup and view all the answers

Redox reactions involve only oxidation or only reduction, but not both.

<p>False (B)</p> Signup and view all the answers

What signifies a reversible reaction in chemical notation?

<p>A double arrow</p> Signup and view all the answers

Electronegativity measures an atom's ability to attract ___________.

<p>electrons</p> Signup and view all the answers

Match the following types of chemical reactions with their definitions:

<p>Double Displacement = Exchange of ions between two compounds Neutralisation = Reaction between an acid and a base Redox = Involves reduction and oxidation Combustion = Reacts with oxygen to produce heat and light</p> Signup and view all the answers

Which of the following increases as you move down a group in the periodic table?

<p>Atomic radius (D)</p> Signup and view all the answers

The periodic table is primarily arranged by increasing atomic mass.

<p>False (B)</p> Signup and view all the answers

What happens to the atomic radius across a period from left to right?

<p>It decreases.</p> Signup and view all the answers

What type of bonding holds together ionic crystals?

<p>Ionic bonds (C)</p> Signup and view all the answers

The ___________ rule indicates that elements in the same group have similar chemical properties.

<p>valence electron</p> Signup and view all the answers

Hydrogen bonds are considered strong intermolecular forces.

<p>False (B)</p> Signup and view all the answers

What is the primary characteristic of simple molecular compounds?

<p>They consist of a few atoms bonded by strong covalent bonds and have weak intermolecular forces.</p> Signup and view all the answers

What characterizes a combustion reaction?

<p>Combines with oxygen to produce heat and light (A)</p> Signup and view all the answers

A giant molecular compound is also known as a ______ because it consists of millions of atoms.

<p>macromolecule</p> Signup and view all the answers

Match the compounds with their properties:

<p>Sodium Chloride = Hard, brittle crystalline solid with high melting point Diamond = One of the hardest substances known Graphite = Used in pencils and lubricating applications</p> Signup and view all the answers

What happens to the properties of simple covalent solids compared to giant molecular compounds?

<p>They typically have very low melting and boiling points. (B)</p> Signup and view all the answers

All elements exhibit allotropy.

<p>False (B)</p> Signup and view all the answers

Name one use of diamond.

<p>Cutting and drilling.</p> Signup and view all the answers

The weak intermolecular forces in simple molecular compounds lead to ______ melting and boiling points.

<p>low</p> Signup and view all the answers

What happens to electronegativity as you move across a period?

<p>It increases (C)</p> Signup and view all the answers

Cations have larger ionic radii compared to their neutral atoms.

<p>False (B)</p> Signup and view all the answers

What is the primary reason for the larger ionic radii of anions?

<p>Increased electron repulsion and additional electrons.</p> Signup and view all the answers

Fluorine is the most electronegative element because it has the most amount of _____ in its group.

<p>protons</p> Signup and view all the answers

Match the type of ion with the explanation of its ionic radius:

<p>Anion = Larger ionic radius due to more electrons and electron repulsion Cation = Smaller ionic radius due to fewer electrons and stronger nuclear pull</p> Signup and view all the answers

Which of the following statements about cations is correct?

<p>They lose electrons (B)</p> Signup and view all the answers

The effective nuclear charge increases when an atom loses electrons.

<p>True (A)</p> Signup and view all the answers

What is the trend in atomic radius as you move down a group?

<p>Atomic radius increases down a group.</p> Signup and view all the answers

The size of the ionic radius of an anion is primarily affected by ______.

<p>electron repulsion</p> Signup and view all the answers

Which factor contributes to the smaller ionic radii of cations?

<p>Loss of electrons (A)</p> Signup and view all the answers

What type of bond forms between hydrogen and a more electronegative atom?

<p>Hydrogen bond (A)</p> Signup and view all the answers

Ionic crystals have weak intermolecular forces holding their structure together.

<p>False (B)</p> Signup and view all the answers

What is the main distinguishing feature between ionic and molecular solids?

<p>Ionic solids are held together by ionic bonds while molecular solids are held together by covalent bonds and weaker intermolecular forces.</p> Signup and view all the answers

The __________ of sodium chloride is a hard, brittle crystalline solid.

<p>structure</p> Signup and view all the answers

Which of the following correctly describes diamond?

<p>One of the hardest substances known (D)</p> Signup and view all the answers

Match the following structures to their properties:

<p>Sodium Chloride = Conducts electricity when dissolved in water Diamond = Used in cutting and drilling Graphite = Used in pencils and lubricants Simple Molecular Compounds = Usually have low melting and boiling points</p> Signup and view all the answers

Simple molecular compounds are typically made up of a large number of atoms bonded together.

<p>False (B)</p> Signup and view all the answers

Compounds that can exist in more than one form in the same physical state are said to exhibit __________.

<p>allotropy</p> Signup and view all the answers

Name a property of graphite that makes it useful.

<p>Graphite is lubricating due to its layered structure allowing sheets to slide over one another.</p> Signup and view all the answers

What is the main product of a neutralisation reaction?

<p>Salt (B)</p> Signup and view all the answers

Combustion reactions are endothermic processes.

<p>False (B)</p> Signup and view all the answers

What does a double arrow in a chemical equation indicate?

<p>Reversible reaction</p> Signup and view all the answers

The atomic radius __________ as you move down a group in the periodic table.

<p>increases</p> Signup and view all the answers

Match the types of reactions with their definitions:

<p>Double Displacement = Two compounds exchange ions Neutralisation = Reaction between an acid and a base Redox = One reactant is oxidised and another is reduced Combustion = Reaction with oxygen producing CO2 and H2O</p> Signup and view all the answers

Which of the following properties tends to decrease as you move across a period?

<p>Atomic radius (A)</p> Signup and view all the answers

What happens to ionic radii when an atom loses electrons to form cations?

<p>Ionic radii decrease because there are fewer electrons (B)</p> Signup and view all the answers

The ability of an atom to attract electrons is known as ionization energy.

<p>False (B)</p> Signup and view all the answers

Which of the following compounds is insoluble in water?

<p>Carbonates (CO32-) (D)</p> Signup and view all the answers

Anions are smaller than their corresponding neutral atoms due to increased electron repulsion.

<p>False (B)</p> Signup and view all the answers

All chlorides are soluble in water.

<p>False (B)</p> Signup and view all the answers

What is the electronegativity trend across a period?

<p>The electronegativity increases across a period.</p> Signup and view all the answers

What defines the trends observed in the periodic table?

<p>Atomic number</p> Signup and view all the answers

What are the two types of forces that influence the structure and properties of elements and compounds?

<p>Intermolecular and Intramolecular forces</p> Signup and view all the answers

Fluorine is considered the most electronegative element because of its strong __________ pull.

<p>nuclear</p> Signup and view all the answers

In double displacement reactions, one or more products typically forms a __________.

<p>precipitate</p> Signup and view all the answers

Which of the following describes the trend of ionization energy as you go down a group?

<p>Decreases (D)</p> Signup and view all the answers

Match the following ions with their corresponding descriptions:

<p>Anions = Negatively charged ions with larger ionic radii Cations = Positively charged ions with smaller ionic radii Electron Repulsion = Result of additional electrons pushing away further Effective Nuclear Charge = Net positive charge experienced by electrons</p> Signup and view all the answers

Metal hydroxides are generally __________ except for those formed with Group 1 and some Group 2 elements.

<p>insoluble</p> Signup and view all the answers

Match the following metal cations with their charge:

<p>Hydrogen = H+ Copper (ii) = Cu2+ Iron (iii) = Fe3+ Calcium = Ca2+</p> Signup and view all the answers

Which of the following anions is associated with sulfate?

<p>Sulfide (S2-) (D)</p> Signup and view all the answers

Van der Waal forces are considered strong intermolecular forces.

<p>False (B)</p> Signup and view all the answers

Which of the following is a characteristic of metallic bonding?

<p>Positive ions are surrounded by mobile electrons. (A)</p> Signup and view all the answers

In a decomposition reaction, a single compound is broken down into multiple products.

<p>True (A)</p> Signup and view all the answers

What law states that matter cannot be created or destroyed in chemical reactions?

<p>Law of conservation of matter</p> Signup and view all the answers

The four different state symbols used in chemical equations are ___, ___, ___, and ___.

<p>aq, s, l, g</p> Signup and view all the answers

What type of reaction involves a more reactive element displacing a less reactive element?

<p>Single Displacement Reaction (B)</p> Signup and view all the answers

Covalent bonds can only form between atoms of different elements.

<p>False (B)</p> Signup and view all the answers

What happens to a compound during a synthesis reaction?

<p>It combines with other substances to form a single product.</p> Signup and view all the answers

In a chemical reaction, products ____ the reactants.

<p>form from</p> Signup and view all the answers

Which of the following does not involve a change in the number of atoms?

<p>Balancing a chemical equation (C)</p> Signup and view all the answers

Flashcards

Double Displacement Reaction

Two compounds in solution swap ions, forming a precipitate (solid) that separates from the solution.

Neutralization Reaction

A reaction between an acid and a base, producing a salt and water.

Redox Reaction

A reaction where one substance is reduced (gains electrons) and another is oxidized (loses electrons).

Periodic Table Arrangement

Elements are arranged by increasing atomic number (number of protons).

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Atomic Radius Trend

Atomic radius increases down a group and slightly decreases across a period.

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Electronegativity

The ability of an atom to attract electrons towards itself in a chemical bond.

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Periodic Table Groups

Elements in the same column (group) have the same number of valence electrons.

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Periodic Law

The properties of elements are periodic functions of their atomic number.

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Group VII: Reactivity

Group VII elements, like chlorine and bromine, readily gain or share one electron to reach a stable electron configuration.

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Group VII: Diatomic Molecules

Group VII elements exist as diatomic molecules (two atoms bonded together) due to their high reactivity. For example, chlorine exists as Cl2.

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Electronegativity Trend in Group VII

Electronegativity decreases as you move down Group VII. This is because the atomic radius increases, making the outer electrons less attracted to the nucleus.

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Period 3 Metals

Metals in Period 3, like sodium and magnesium, have a range of properties, including good conductivity and malleability.

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Period 3 Nonmetals

Period 3 nonmetals, like chlorine and phosphorus, are typically gases or brittle solids, with low conductivity.

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Predicting Element Properties

By knowing an element's position on the periodic table, you can predict its general properties, such as whether it's a metal or nonmetal, its reactivity, and its state at room temperature.

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What happens to reactivity down Group VII?

The reactivity of Group VII elements, like chlorine and bromine, decreases as you move down the group.

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What are the key properties of metals in Period 3?

Metals in Period 3, like sodium and magnesium, are generally good conductors of heat and electricity, have high melting points, and are malleable.

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Effective Nuclear Charge

The net positive charge experienced by an electron in an atom, taking into account the shielding effect of inner electrons.

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Shielding Effect

The reduction in the effective nuclear charge felt by outer electrons due to the repulsion from inner electrons.

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Ionization Energy Trend: Down a Group

Ionization energy decreases as you move down a group in the periodic table because the increased size and shielding effect make valence electrons easier to remove.

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Ionization Energy Trend: Across a Period

Ionization energy increases across a period in the periodic table because the increased effective nuclear charge makes valence electrons harder to remove.

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Oxidizing Agent

A substance that gains electrons in a chemical reaction, causing another substance to lose electrons (oxidize).

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Reducing Agent

A substance that loses electrons in a chemical reaction, causing another substance to gain electrons (reduce).

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Metal Reactivity Trend: Down a Group

Metals become more reactive as you move down a group. This is because their atomic size increases, making it easier to lose valence electrons.

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Group II Elements

Group II elements, known as alkaline earth metals, are reactive metals that readily lose their two valence electrons to form +2 ions. They include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).

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Ionic Bonds

A type of chemical bond formed between atoms due to the electrostatic attraction between oppositely charged ions. It occurs between a metal (which tends to lose electrons) and a non-metal (which tends to gain electrons).

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Covalent Bonds

A type of chemical bond formed between atoms by the sharing of valence electrons. This type of bond typically occurs between two or more non-metal atoms.

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Lone Pairs

Pairs of valence electrons in an atom that are not involved in bonding with other atoms.

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What are the common elements in covalent bonds?

Covalent bonds usually occur between two or more non-metal atoms.

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What makes fluorine a molecule?

Fluorine, being a halogen, has 7 valence electrons, making it eager to gain one electron for a stable configuration. It forms a bond with another fluorine atom by sharing their lone pairs, thus creating the fluorine molecule, F2.

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Why are there lone pairs in fluorine?

Fluorine atoms have 7 valence electrons. They need 8 electrons to reach a stable configuration. They form a bond with another fluorine atom by sharing one electron, but still have 3 pairs of electrons that aren't involved in bonding, hence the lone pairs.

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What is the difference between ionic and covalent bonds?

Ionic bonds transfer electrons between the metal and non-metal, leading to the formation of positively and negatively charged ions, which attract each other. Covalent bonds involve sharing of electrons between two or more non-metal atoms to achieve a stable electron configuration.

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Hydrogen Bond

A weak attraction between a hydrogen atom covalently bonded to a highly electronegative atom (like oxygen or nitrogen) and a lone pair of electrons on another electronegative atom in a different molecule.

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Intermolecular Forces

Weak attractions between molecules, affecting physical properties like melting and boiling points.

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Ionic Crystals

Solids formed by repeating, three-dimensional arrays of positively and negatively charged ions held together by strong electrostatic attractions.

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Simple Molecular Compounds

Compounds formed by a small number of atoms covalently bonded together, with weak intermolecular forces holding the molecules together. They usually have low melting and boiling points.

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Giant Molecular Compounds

Compounds formed by a vast network of atoms covalently bonded in a three-dimensional structure. They are strong and have high melting points.

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Sodium Chloride Structure

A regular, three-dimensional lattice structure with alternating sodium (Na+) and chloride (Cl-) ions held together by strong ionic bonds.

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Diamond Structure

Each carbon atom is tetrahedrally bonded to four other carbon atoms forming a strong, three-dimensional network.

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Graphite Structure

Each carbon atom is bonded to three other carbon atoms, forming flat sheets that are weakly held together. This allows the sheets to slide easily over each other, giving graphite its lubricating properties.

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Allotropy

The ability of an element to exist in more than one physical form, with different structures and properties.

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Ionisation Energy

The minimum energy needed to remove one electron from a neutral atom in the gaseous state.

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1st Ionisation Energy

The energy required to remove the first (outermost) valence electron from a neutral atom in the gaseous state.

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Factors Affecting Ionisation Energy

Three main factors influence ionisation energy: distance of valence electrons from the nucleus, effective nuclear charge, and shielding effect.

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Reversible Reaction

A reaction where the direction of the chemical change can be reversed easily. Shown with double arrows.

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Combustion Reaction

A reaction where oxygen combines with a compound, forming carbon dioxide and water, releasing heat.

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Electronegativity Trend

Electronegativity decreases down a group and increases across a period. It's the atom's ability to attract electrons in a bond.

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Electronegativity and Atomic Radii

Electronegativity is inversely proportional to atomic radius. This means a smaller atom with a strong pull on its electrons will be more electronegative.

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Fluorine & Electronegativity

Fluorine is the most electronegative element. It's the strongest electron 'thief' because it has a small size and large nuclear charge.

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Ionic Radii of Anions

Anions (negatively charged ions) have larger ionic radii than their neutral atoms. They gain electrons, increasing repulsion and reducing effective nuclear charge.

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Ionic Radii of Cations

Cations (positively charged ions) have smaller ionic radii than their neutral atoms. They lose electrons, reducing repulsion and increasing effective nuclear charge.

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Electron Repulsion

Electron repulsion is the force experienced between negatively charged electrons. It contributes to ionic radii size.

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Explain the trend of electronegativity and ionic radii

Electronegativity decreases down a group because atomic radii increases, weakening the pull of the nucleus on outer electrons. Across a period, electronegativity increases because atomic radii decreases, strengthening the pull on outer electrons. However, ionization energy increases as you move right across the period.

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Solubility Rules

Guidelines predicting whether a compound will dissolve in water based on its cation and anion.

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Group 1 Elements & Solubility

Group 1 elements (Li+, Na+, K+) form soluble compounds with most anions.

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Nitrates & Solubility

Nitrates (NO3-) form soluble compounds with most cations.

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Insolubility Rules

Guidelines predicting which compounds will not dissolve in water.

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Metal Hydroxides & Insolubility

Most metal hydroxides (OH-) are insoluble, except for Group 1 elements and a few Group 2 elements.

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Carbonates & Insolubility

Most carbonates (CO32-) are insoluble, with exceptions for Group 1 elements and ammonium (NH4+).

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Sulphides & Insolubility

Most sulphides (S2-) are insoluble, except for Group 1 elements, Group 2 elements, and ammonium (NH4+).

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What is a chemical reaction?

A process where atoms rearrange to form new substances.

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Law of Conservation of Matter

Matter cannot be created or destroyed in chemical reactions, only rearranged.

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State Symbols

Represent the physical state of a substance in a reaction: (s) solid, (l) liquid, (g) gas, (aq) dissolved in water.

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Synthesis Reaction

Two or more substances combine to form a single product.

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Decomposition Reaction

A single compound breaks down into two or more products.

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Single Displacement Reaction

A more reactive element replaces another element in a compound.

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Coordinate Covalent Bond

Both electrons in the bond come from the same atom.

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Metallic Bonding

Electrons are mobile, creating a 'sea' that holds positive metal ions together.

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Weak Intermolecular Forces

Forces between molecules, much weaker than bonds within molecules.

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Giant Metallic Structure

Metals form a giant, three-dimensional structure with mobile electrons.

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Atomic Radii and Electronegativity

Electronegativity is inversely proportional to atomic radii. A smaller atom with a stronger pull on its electrons will be more electronegative.

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Fluorine: The Most Electronegative

Fluorine is the most electronegative element on the periodic table. It has a small size and a large nuclear charge, which allows it to attract electrons very strongly.

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Ionic Radii: Anions vs. Cations

Anions (negatively charged ions) are larger than their neutral atoms. They have gained electrons, increasing electron repulsion and reducing the effective nuclear charge. Cations (positively charged ions) are smaller than their neutral atoms. They have lost electrons, reducing repulsion and increasing the effective nuclear charge.

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How do electron repulsion and effective nuclear charge affect ionic radii?

Electron repulsion is the force between the electrons of an atom. When an atom gains electrons (anion), increased repulsion forces the electrons further apart, making the ionic radius larger. When an atom loses electrons (cation), reduced repulsion allows the remaining electrons to be pulled closer to the nucleus, making the ionic radius smaller. Effective nuclear charge is the net positive charge felt by outer electrons. This is affected by the shielding effect of inner electrons. A weaker effective nuclear charge leads to a larger ionic radius, while a stronger effective nuclear charge leads to a smaller ionic radius.

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Ionization Energy Trend

Ionization energy decreases down a group and increases across a period.

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Study Notes

CHEM EXAM 2024: THE CHEMICAL AWAKENS

  • Exam scheduled for December 10th
  • Exam duration: 1 hour and 45 minutes

Topics

  • Chemistry Lab, Laboratory Equipments & Safety Regulations

    • Planning and Designing Experiments
      • Identifying and creating questions and hypotheses
      • Developing experimental procedures
      • Analyze various variables in investigations.
      • Analyze evidence, infer, make predictions, and explain observations.
      • Presenting quantitative data in scientific investigations.
      • Strengths and weaknesses of arguments and/or claims.
    • Chemical Bonding and Structure
      • Ionic Bonds
        • Forces of attraction due to ions of opposite charges
        • Occur between metals (which tend to lose electrons) and nonmetals (which tend to gain electrons)
      • Covalent Bonds
        • Bond formation through valence electron sharing between nonmetals.
        • Resulting in molecule formation
        • Examples: water (Hâ‚‚O), hydrogen (Hâ‚‚), oxygen (Oâ‚‚)
      • Lone pairs (non-bonding pairs): Electrons not directly involved in bonding.

  • Predict likelihood of ionic/covalent bonds based on atomic structure

  • Write formulae to represent ions and molecules

  • Chemical and Ionic Equations

    • Equations are a shorthand representation of reactions.
    • Ionic equations indicate participating atoms that change state.

  • Solubility & Insolubility Rules

    • Rules for predicting the solubility of compounds in water.
    • Compound categories and exceptions in solubility.

  • Polyatomic Ions

  • Cations and Anions

  • Types of Covalent Bonds

    • Single, double, triple bonds

  • Intra- and Inter-molecular forces

    • Properties based on attractive & repulsive forces within and between molecules.
    • van der Waals forces: Weak forces between oppositely-charged ends of molecules.

  • Structure And Properties of Ionic, Simple Molecular and Giant Molecular Crystals

    • Sodium Chloride (NaCl), Diamond, Graphite

  • Allotropes: Different forms of the same element in the same physical state.

  • Periodicity

    • Trends in atomic radius, ionization energy, and electronegativity.

  • Periodic Table

    • Arrangement of elements based on atomic number (protons.)
    • Group trends in reactivity, properties, and bonding.

  • Trends in Period 3

  • Chemical Reactivity

    • Understanding reactions with oxygen, water, and acids.

  • Types of Reactions

    • Decomposition, Single Displacement, Double Displacement, Neutralization, Redox
    • Balancing chemical equations.

  • Predicting Properties of Elements Based on Position in the Periodic Table

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