Chemistry Chapter on Ionic Compounds
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Questions and Answers

Which of the following non-metals has a charge of 2-?

  • SO4 (correct)
  • Cl
  • O (correct)
  • Br

Sodium (Na) is a non-metal.

False (B)

What charge does calcium (Ca) typically have in ionic compounds?

2+

The formula for the ammonium ion is ______.

<p>NH4+</p> Signup and view all the answers

Match the following metals with their typical charges:

<p>Cu(I) = 1+ Fe(II) = 2+ Al = 3+ Zn = 2+</p> Signup and view all the answers

What is a physical state of substances that has a high melting and boiling point?

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

Sodium chloride can conduct electricity when it is solid.

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

Why are metals generally considered to be good conductors of electricity?

<p>Metals have free-moving electrons that facilitate the flow of electrical current.</p> Signup and view all the answers

Sodium chloride has __________ solubility in water.

<p>good with exceptions</p> Signup and view all the answers

Match the following substances with their respective solubility in non-polar solvents:

<p>Sodium chloride = Poor Methane = Good Copper sulfate = None Ethanol = None</p> Signup and view all the answers

Which of the following compounds will only conduct electricity when molten or in aqueous solution?

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

Aluminium bronze has lower resistance to corrosion than pure copper.

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

What allows metals to be ductile?

<p>The ability of atoms to slide past each other without breaking bonds.</p> Signup and view all the answers

What type of bond involves the transfer of electrons from metal to non-metal?

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

Covalent compounds generally have high melting and boiling points.

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

What is formed when substances combine with oxygen?

<p>Oxidised substances</p> Signup and view all the answers

Ionic compounds are solid at room temperature and have _____ melting and boiling points.

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

Match the following properties with the correct type of bond:

<p>High melting points = Ionic Compound Low melting points = Covalent Compound Charges present = Ionic Compound No charges = Covalent Compound</p> Signup and view all the answers

Which of the following describes the structure of ionic compounds?

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

Ionic compounds can conduct electricity in their solid state.

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

What are the weak forces of attraction between molecules in covalent compounds called?

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

Ionic compounds are usually soluble in water unless they _____ with the water.

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

Which of the following compounds contains calcium?

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

Only non-metal atoms can form covalent bonds.

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

What is the electron structure of hydrogen?

<p>1</p> Signup and view all the answers

In a fluorine molecule (F2), two fluorine atoms share __________ electrons.

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

Match the following chemical compounds with their formula:

<p>Calcium chloride = CaCl2 Copper (II) nitrate = Cu(NO3)2 Zinc nitrate = Zn(NO3)2 Sodium hydroxide = NaOH</p> Signup and view all the answers

What is the main characteristic of covalent bonds?

<p>Sharing of electrons (D)</p> Signup and view all the answers

In a covalent bond, atoms are held together by the attraction of electrons to their nuclei.

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

How many outer electrons are in a fluorine atom?

<p>7</p> Signup and view all the answers

What is the main purpose of the tests described in the document?

<p>All of the above (D)</p> Signup and view all the answers

The appearance of substances can provide information about the arrangement of their particles.

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

What suggestion is made regarding the melting points of substances in relation to their bonding?

<p>Higher melting points suggest stronger bonds between particles.</p> Signup and view all the answers

If a solid substance conducts electricity, this indicates that the particles are ______.

<p>charged or mobile</p> Signup and view all the answers

Which of the following is used to test the solubility of a substance?

<p>Beakers with water and propanone (B)</p> Signup and view all the answers

Match the following properties with their corresponding tests:

<p>Appearance = Color and state Conductivity = Electricity flow Melting point = Heat application Solubility = Dissolving in solvent</p> Signup and view all the answers

Water is considered a good solvent for all substances.

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

The outcome of whether a solution conducts electricity can indicate the presence of ______ in the solution.

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

What is the molar mass of magnesium nitrate, Mg(NO3)2?

<p>148 g/mole (C)</p> Signup and view all the answers

The molar mass of water is 24 g/mole.

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

What is the formula for calculating the number of moles from mass and molar mass?

<p>Moles = mass / molar mass</p> Signup and view all the answers

The molar mass of copper (II) oxide, CuO, is _____ g/mole.

<p>79.5</p> Signup and view all the answers

Match the following compounds with their molar masses:

<p>Copper (II) Sulphate = 160 g/mole Zinc Carbonate = 125 g/mole Ammonium Carbonate = 96 g/mole Sulphur Trioxide = 80 g/mole</p> Signup and view all the answers

How many moles are in 40 g of copper (II) sulphate, CuSO4?

<p>0.5 moles (B)</p> Signup and view all the answers

An ionic compound generally has higher melting points compared to covalent compounds.

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

If you have 0.1 moles of sulphur trioxide, what mass do you have?

<p>8 g</p> Signup and view all the answers

Flashcards

Covalent Bonding

A type of chemical bond formed when two non-metal atoms share electrons to achieve a stable electron configuration.

Electron Sharing

The process where non-metal atoms share their outermost electrons to achieve a stable electron configuration similar to a noble gas.

Inert Gas Configuration

A stable electron configuration where atoms have a full outermost energy level, making them unreactive.

Hydrogen Molecule (H2)

Two hydrogen atoms share one electron each, forming a covalent bond and achieving a stable electron configuration.

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Fluorine Molecule (F2)

Two fluorine atoms share one electron each, resulting in a stable electronic configuration similar to Neon.

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Bonding Diagram

A visual representation of how electrons are shared in a covalent bond, showing the arrangement of atoms and their shared electrons.

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Structural Formula

A simplified representation of a molecule, showing only the atoms and the bonds between them.

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Molecular Formula

A representation of a molecule showing the types and number of atoms present.

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Molar Mass

The mass of one mole of a substance, expressed in grams per mole (g/mol). It represents the mass of 6.022 x 10^23 particles (atoms, molecules, or ions) of that substance.

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How to calculate Molar Mass?

Add the atomic masses of all the atoms in a molecule. Use the periodic table to find the atomic mass of each element.

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Moles

A unit of measurement for the amount of substance. One mole contains 6.022 x 10^23 particles (Avogadro's number).

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Calculating Moles

Divide the mass of the substance by its molar mass. This tells you how many moles of the substance are present.

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Calculating Mass

Multiply the number of moles by the molar mass. This gives you the mass of the substance in grams.

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Copper (II) Oxide Formula

CuO

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Sulphur Trioxide Formula

SO3

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Ammonium Carbonate Formula

(NH4)2CO3

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What does the appearance of a substance tell us about its particles?

The appearance of a substance (solid, liquid, powder, etc.) gives clues about how its particles are arranged. Solids have tightly packed particles, liquids are less tightly packed, and gases have very loosely packed particles.

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What does the effect of heat on a substance tell us about its bonding?

Heating a substance can break the bonds between its particles. The stronger the bonds, the more energy is needed to break them and the higher the melting point.

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What does electrical conductivity tell us about a substance's particles?

Substances that conduct electricity have free-moving charged particles (electrons or ions). Solids that conduct electricity have free electrons, while solutions with dissolved ions conduct due to the movement of ions.

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How does solubility affect a substance's conductivity?

When a substance dissolves, its particles become surrounded by solvent molecules. If these particles are ions, the solution conducts electricity.

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What influences the choice of solvent?

The choice of solvent depends on the substance's properties and the type of interactions between the substance's particles and the solvent molecules.

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What does a substance's solubility tell us about the forces between its particles?

The solubility of a substance (how well it dissolves) is related to the strength of the forces between its particles and the solvent particles. Stronger forces mean lower solubility.

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What is propanone used for?

Propanone, also known as acetone, is a common solvent used in many applications. It's used in nail polish remover due to its ability to dissolve many types of polymers.

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What is cyclohexane used for?

Cyclohexane is a non-polar solvent that is used in a variety of applications, including the extraction of organic compounds.

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Ionic Compound Formula

The formula representing the ratio of ions in a stable ionic compound. It reflects the charges and balancing of positive and negative ions.

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Metal Ions

Positively charged ions formed when metal atoms lose electrons. They typically have a fixed charge, depending on the metal's position in the periodic table.

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Non-Metal Ions

Negatively charged ions formed when non-metal atoms gain electrons. Their charge varies based on the number of electrons gained.

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How to Predict the Formula?

Determine the charges of the metal and non-metal ions, then use the criss-cross method to find the smallest whole-number ratio of ions needed to balance the charges.

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Charge Balance

The total positive charge from metal ions must be equal to the total negative charge from non-metal ions in a stable ionic compound.

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Giant Ionic Structure

A structure formed by a strong electrostatic attraction between oppositely charged ions arranged in a regular, repeating pattern.

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Giant Covalent Structure

A structure where atoms are strongly bonded together in a continuous network by sharing electrons.

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Molecular Structure

A structure composed of discrete molecules, where atoms are held together by covalent bonds within each molecule.

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Metals - Good Conductors of Electricity

Metals have a sea of delocalized electrons which can move freely, allowing them to conduct electricity easily.

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Metals - High Densities

Metals have closely packed atoms in a regular arrangement, making them dense.

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Methane - Gas at Room Temperature

Methane is a small molecule with weak intermolecular forces, making it a gas at room temperature.

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Sodium Chloride - Conducts Electricity When Molten or in Solution

Ionic compounds like sodium chloride only conduct electricity when their ions are free to move, which happens when melted or dissolved in water.

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Ductile Metals

Metals that can be drawn into wires due to the ability of their atoms to slide over each other.

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Giant ionic lattice

A repeating pattern of positively and negatively charged ions in an ionic compound, forming a crystal structure.

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Intermolecular forces

Weak forces of attraction between molecules in a covalent compound, determining its physical state (solid, liquid, or gas).

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Why do covalent compounds have low melting points?

Covalent compounds have weak intermolecular forces, requiring less energy to break the bonds and change their state of matter.

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Why are covalent compounds usually non-conductors?

Covalent compounds don't have free-moving ions or electrons to carry an electric current.

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Ionic Compound

A compound formed by the transfer of electrons between a metal and a non-metal, resulting in a positive and negative ion.

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Covalent Compound

A compound formed by the sharing of electrons between two non-metal atoms.

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Oxidation

A chemical process where a substance gains oxygen atoms or loses electrons.

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Reduction

A chemical process where a substance loses oxygen atoms or gains electrons.

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Study Notes

Bonding

  • Ionic Bonding: Ionic bonds form between oppositely charged ions. Positive ions (cations) and negative ions (anions) attract each other due to electrostatic forces creating a giant lattice structure. Common examples involve metals from Groups I and VII.
  • Properties of Ionic Compounds:
    • High melting and boiling points due to strong electrostatic forces.
    • Good electrical conductivity in molten or aqueous states, but poor in solid state (ions are fixed in place).
    • Generally soluble in water.
  • Covalent Bonding: Covalent bonds form when atoms share electron pairs to achieve a stable electron configuration (similar to noble gases). The shared electrons are attracted to the nuclei of both atoms, holding them together. This type of bonding occurs in simple molecules.
  • Properties of Simple Molecular Compounds:
    • Low melting and boiling points due to weak intermolecular forces.
    • Poor electrical conductivity in all states due to no mobile charge carriers.
  • Giant Covalent Structures: Giant covalent structures are formed when atoms are covalently bonded together in a continuous network.
    Diamond (hard and high melting point) and graphite (soft and lubricant) are examples of such structures.
  • Metallic Bonding: Positive metal ions are held in a lattice surrounded by a 'sea' of delocalized electrons. These mobile electrons allows for good electrical and thermal conductivity, ductility and malleability, as well as high melting points.
  • Formulas: Chemical formulas represent the ratio of atoms in a molecule (simple molecular) or the relative numbers of ions (ionic). Use valencies to obtain the correct formula.

Formulas

  • Chemical formulas represent the ratio of atoms in a molecule (simple molecular) or the relative numbers of ions (ionic).
  • Use valencies to obtain the correct formula. The charges will cancel out.

Relative Atomic Mass

  • Defined as the average mass of atoms of an element compared to 1/12th the mass of a carbon-12 atom.

Redox

  • Oxidation: Gain of oxygen/loss of electrons, an increase in oxidation number.
  • Reduction: Loss of oxygen/gain of electrons, a decrease in oxidation number.
  • Redox reactions involve both oxidation and reduction occurring simultaneously.

Moles

  • A mole is a unit of measurement for the amount of substance (6.02 x 10²³ particles).
  • Molar mass is the mass of one mole of a substance in grams.
  • The molar mass of a compound equals the sum of the relative atomic masses (Ar) of the component atoms.
  • Moles = mass / molar mass

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Test your knowledge on ionic compounds and their properties with this comprehensive quiz. Questions cover charges, conductivity, solubility, and bonding types relevant to non-metals and metals. Ideal for students studying chemistry topics related to ionic and covalent compounds.

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