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Questions and Answers
Which of the following is a characteristic property of metals?
Which of the following is a characteristic property of metals?
What is the term used to describe compounds that do dissolve in water?
What is the term used to describe compounds that do dissolve in water?
Non-metallic oxides are typically basic in nature.
Non-metallic oxides are typically basic in nature.
False (B)
What type of charge do ions of metals typically have?
What type of charge do ions of metals typically have?
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Ionic compounds do not separate into ions when they dissolve in water.
Ionic compounds do not separate into ions when they dissolve in water.
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Metals are said to be ______, meaning they can be beaten into shape.
Metals are said to be ______, meaning they can be beaten into shape.
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Name an example of an ionic compound.
Name an example of an ionic compound.
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Match the following elements with their state at room temperature:
Match the following elements with their state at room temperature:
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Compounds that do not dissolve in water are described as ______.
Compounds that do not dissolve in water are described as ______.
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What is the term used to describe the bonding that occurs within a sample of a metal?
What is the term used to describe the bonding that occurs within a sample of a metal?
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Match the following terms with their definitions:
Match the following terms with their definitions:
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All metals are solids at room temperature.
All metals are solids at room temperature.
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In the structure of a typical metal, what surrounds the closely packed metal ions?
In the structure of a typical metal, what surrounds the closely packed metal ions?
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What type of bond is formed between cations and electrons in metals?
What type of bond is formed between cations and electrons in metals?
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What gas is identified by the pop-test?
What gas is identified by the pop-test?
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Metals tend to gain electrons in chemical reactions.
Metals tend to gain electrons in chemical reactions.
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What is the electron configuration of a Na^+ ion?
What is the electron configuration of a Na^+ ion?
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Oxygen gas can be identified by its reaction with a glowing wooden splint which relights in oxygen.
Oxygen gas can be identified by its reaction with a glowing wooden splint which relights in oxygen.
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What happens to limewater when carbon dioxide is passed into it?
What happens to limewater when carbon dioxide is passed into it?
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The cations in a metallic lattice are surrounded by a sea of ______ electrons.
The cations in a metallic lattice are surrounded by a sea of ______ electrons.
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Which of the following metals is considered highly reactive?
Which of the following metals is considered highly reactive?
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The chemical reaction for burning hydrogen is represented as 2H2 + O2 → 2H2O + _____
The chemical reaction for burning hydrogen is represented as 2H2 + O2 → 2H2O + _____
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Match the following metals with their electron loss characteristics:
Match the following metals with their electron loss characteristics:
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Match the metals with their corresponding flame test colors:
Match the metals with their corresponding flame test colors:
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What is the by-product of the combustion of hydrogen?
What is the by-product of the combustion of hydrogen?
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Aluminium loses one electron to become Al^3+.
Aluminium loses one electron to become Al^3+.
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Calcium bicarbonate is insoluble in water.
Calcium bicarbonate is insoluble in water.
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What is the electron arrangement for a Ca^2+ ion?
What is the electron arrangement for a Ca^2+ ion?
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What is the purpose of a flame test?
What is the purpose of a flame test?
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Which of the following describes covalent lattices?
Which of the following describes covalent lattices?
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All atoms in a covalent lattice are freely mobile.
All atoms in a covalent lattice are freely mobile.
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What is a property of substances with strong covalent bonds that affects their electrical conductivity?
What is a property of substances with strong covalent bonds that affects their electrical conductivity?
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Covalent lattices may be ______ or layered structures.
Covalent lattices may be ______ or layered structures.
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Which of the following is a characteristic of hydrogen bonding?
Which of the following is a characteristic of hydrogen bonding?
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Match the type of bond or interaction with its characteristic.
Match the type of bond or interaction with its characteristic.
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What is the significance of delocalized electrons in graphite?
What is the significance of delocalized electrons in graphite?
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The formula for sulfur dioxide is ______.
The formula for sulfur dioxide is ______.
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How many valence electrons does carbon have?
How many valence electrons does carbon have?
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O=C=O represents a molecule where carbon has a full valence shell.
O=C=O represents a molecule where carbon has a full valence shell.
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What problem arises when distributing the valence electrons around the carbon atom?
What problem arises when distributing the valence electrons around the carbon atom?
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In order for a carbon atom to achieve a full valence shell, it needs to move a non-bonding electron pair from a __________ atom.
In order for a carbon atom to achieve a full valence shell, it needs to move a non-bonding electron pair from a __________ atom.
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Match the following descriptions to their corresponding processes:
Match the following descriptions to their corresponding processes:
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What happens to the non-bonding electron pairs during the bonding process?
What happens to the non-bonding electron pairs during the bonding process?
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The total number of electrons used in this process is less than 16.
The total number of electrons used in this process is less than 16.
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What is the structural formula when double bonds are formed in this example?
What is the structural formula when double bonds are formed in this example?
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Flashcards
Metals as conductors
Metals as conductors
Metals are good conductors of heat and electricity.
Non-metals as insulators
Non-metals as insulators
Non-metals are thermal and electrical insulators.
Strength of metals
Strength of metals
Metals typically have high strength.
Brittleness of non-metals
Brittleness of non-metals
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Malleability and ductility of metals
Malleability and ductility of metals
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Metallic oxides
Metallic oxides
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Non-metallic oxides
Non-metallic oxides
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Ionic charges of metals
Ionic charges of metals
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Metallic Bonding
Metallic Bonding
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Cations
Cations
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Delocalized Electrons
Delocalized Electrons
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Electron Configuration
Electron Configuration
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Reactivity of Metals
Reactivity of Metals
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Noble Gas Configuration
Noble Gas Configuration
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Valence Electrons
Valence Electrons
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Chemical Reactivity Patterns
Chemical Reactivity Patterns
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Carbon's Valence Electrons
Carbon's Valence Electrons
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Total Electrons in Carbon Compound
Total Electrons in Carbon Compound
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Distributing Electrons
Distributing Electrons
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Full Valence Shell
Full Valence Shell
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Non-bonding Electron Pair
Non-bonding Electron Pair
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Double Bonds
Double Bonds
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Electron Dot Diagram
Electron Dot Diagram
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Ionic Compounds
Ionic Compounds
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Dissolution of NaCl
Dissolution of NaCl
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Soluble vs Insoluble
Soluble vs Insoluble
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Ionic Bonds
Ionic Bonds
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Solubility Table
Solubility Table
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Pop test for hydrogen
Pop test for hydrogen
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Limewater test for CO₂
Limewater test for CO₂
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Oxygen ignition test
Oxygen ignition test
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Unknown ionic compound detection
Unknown ionic compound detection
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Flame test for metals
Flame test for metals
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Barium flame test color
Barium flame test color
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Calcium flame test color
Calcium flame test color
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Flame Emission Spectroscopy
Flame Emission Spectroscopy
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Covalent Bonds
Covalent Bonds
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Intermolecular Forces
Intermolecular Forces
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Hydrogen Bonding
Hydrogen Bonding
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Covalent Lattices
Covalent Lattices
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Conductivity in Lattices
Conductivity in Lattices
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MP and BP in Lattices
MP and BP in Lattices
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3D and 2D Structures
3D and 2D Structures
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Study Notes
Chemical Structures and Properties (Criterion 7)
- Chemical properties and the structures of atoms
- The Periodic Table is structured based on electron configuration.
- Elements in the same period or group have similar properties and reactivity.
- Elements are organized into metals and non-metals.
- Groups 1, 2, 17, and 18 have similar properties and common ionic charges.
- Reactivity trends are observed in periods 2 and 3, and groups 1, 2, and 17.
- Atomic properties, including bond formation, are explained by electron configurations.
Properties and Structures of Materials
- The type of bonding determines the physical properties of a substance.
- Metallic, ionic, and covalent substances have different structures and properties.
- Chemical bonds form due to electrostatic attractions resulting from electron sharing or transfer.
- Valency is a measure of the number of bonds an atom can form.
- Ions are electrically charged atoms. Ionic bond formulas show constituent elements and charge.
- Ionic compounds have high melting points, are brittle, and conduct electricity when molten or dissolved.
- Metallic bonding involves a lattice of positively charged ions surrounded by mobile electrons.
- Metallic properties (malleability, thermal/electrical conductivity) are due to this model.
- Covalent substances are molecules or networks.
- Intramolecular forces (strong bonds) are within molecules, while intermolecular forces (weak bonds) are between molecules.
- Electron dot diagrams represent simple molecular compounds.
Chemical Properties of Metals
- Metals tend to lose electrons to form positive ions (cations), reacting with various chemical compounds.
- Losing electrons results in a similar electron configuration to a noble gas.
- Reactivity varies among metals; some lose electrons more easily (highly reactive).
Comparing Metals and Nonmetals
- Metals are lustrous, typically solid at room temperature, with high densities.
- Good conductors of heat and electricity
- Malleable and ductile.
- Metallic oxides are basic.
- Nonmetals are not lustrous, can be solids, liquids, or gases, with low densities.
- Poor conductors of heat and electricity.
- Brittle in solid form.
- Nonmetallic oxides are acidic.
Metallic Bonding
- Metallic bonding describes the bonding in metals.
- A metal lattice structure consists of closely packed metal ions surrounded by a 'sea' of delocalised electrons.
- Electrostatic attractions between these ions and electrons result in strong bonding, explaining high melting points, malleability, and ductility.
Properties of Metals
- Malleability and ductility are possible because of the delocalised electrons.
- Metals can conduct heat due to the delocalised electrons.
- Lustre is caused by the presence of free electrons.
Chemical Properties of Metals
- Metals react by losing electrons forming positive ions. (Cations)
- The result is the same electron configuration as a noble gas.
- Some metals lose electrons more easily than others, resulting in wide variance in reactivity.
Reactivity of Metals
- Reactivity of metals generally increases as you move down a group, like group 1 (alkali metals).
- As atomic radius increases down a group in metals, the valence electrons are further away from the nucleus, causing less attraction, making the metals more reactive.
Elements and the Periodic Table: Semi-metals
- Semi-metals have properties that are intermediate between metals and nonmetals.
- Some examples of semi-metals include boron, silicon, germanium, etc.
Elements and the Periodic Table: Nonmetals
- Nonmetals are generally poor electrical and thermal conductors and are typically not lustrous or malleable.
- They exist as solids, liquids or gases at room temperature.
- The reactivity of nonmetals varies considerably as you move down a given group.
Bonding and Chemical Compounds
- Chemical compounds are composed of two or more elements chemically bonded together.
- Chemical compounds have constant composition and properties.
- Ionic compounds are formed by the attraction between positive and negative ions.
- Covalent compounds contain covalent bonds and are formed when atoms share electrons.
Ionic Compounds (Naming and Formulae)
- Naming involves writing the cation (metal) first, followed by the anion (non-metal) with an ‘ide’ ending, sometimes with Roman Numerals for transition metals.
- Formulas balance positive and negative charges. Use the number of each ion in the chemical formula.
Ionic Compounds Containing Polyatomic Ions
- Polyatomic ions are groups of atoms with a charge.
- Names for polyatomic ions are fixed (for example, sulfate (SO42-), nitrate (NO3-), ammonium (NH4+)).
- For compounds with polyatomic ions, place the polyatomic ion in parentheses if there is more than one of the polyatomic ion in the formula.
Covalent Compounds (Naming and Formulae)
- Naming prefixes denote the number of atoms. Use prefixes to denote the number of atoms in the chemical formula. e.g. CO2 = carbon dioxide and N₂O₄ = dinitrogen tetroxide.
The Structure of Ionic Compounds
- Ionic compounds are 3-dimensional crystal lattices, not molecules, with repeating arrays of alternating cations and anions held together by electrostatic attraction.
- High melting and boiling points due to strong electrostatic forces.
- Hard but brittle. Not good conductors in solid form. Good conductors when dissolved in liquid or as aqueous solutions.
Covalent Compounds – Structures and Bonding
- Most covalent compounds are molecules that consist of discrete atoms.
- Covalent molecules have weak intermolecular forces (e.g., dispersion forces, sometimes dipole-dipole interactions, and hydrogen bonds) between molecules that influence melting and boiling points and other properties.
- Covalent lattices may form 3-dimensional networks.
- Strong covalent bonds throughout the lattice give them high melting points and inertness, like diamond.
Covalent Bonding: Different Elements
- The sharing of electrons in covalent bonds leads to molecules of specific shapes, and these have properties that are different from ionic or metallic compounds.
- Diatomic nonmetals form molecules in which two atoms share electron pairs to achieve a full outer shell. For instance, chlorine forms Cl2 molecules via a single electron pair shared between chlorine atoms.
- Oxygen forms O2 molecules by sharing two pairs of electrons (double bond).
Covalent Bonding: Drawing Diagrams (Lewis diagrams)
- Lewis structures use valence electrons only to show bonding atoms and unbonded electron pairs.
- The goal is to achieve a full outer electron shell (octet rule) for each atom, except hydrogen.
Forces in Covalent Molecular Bonding
- Dispersion forces are weak attractive forces that emerge from temporary changes in electron density within molecules.
- Polar molecules additionally have dipole-dipole attractions resulting from permanent partial positive and negative charges, and these often lead to higher boiling points than non-polar compounds.
Types of Formulae
- Molecular formula shows the exact number of atoms.
- Empirical formula shows the simplest ratio of atoms.
- Structural formula shows the bonds.
- Semi-structural formula shows some bonds but not all
Isomerism
- Isomers have the same molecular formula but different structures.
- Variations arise from differing arrangements of atoms. Different isomer forms result in difference of properties.
Homologous Series of Hydrocarbons
- A homologous series of hydrocarbons shows a pattern of recurring structural units, which leads to similar chemical and physical properties within the homologous series.
- These are classified as alkanes, alkenes, or alkynes, depending on whether they have single, double, or triple bonds, respectively.
Combustion of Hydrocarbons
- Complete combustion in plentiful oxygen produces carbon dioxide and water.
- Incomplete combustion in limited oxygen yields carbon monoxide and potentially carbon, as well as water.
Tests for Unsaturation
- Bromine water decolorization is used to distinguish saturated from unsaturated hydrocarbons.
- Saturated hydrocarbons typically do not decolorize bromine water, while unsaturated ones react rapidly, producing a colorless compound.
Naming Organic Compounds (IUPAC Nomenclature)
- Organic compounds are systematically named using the IUPAC system, which uses prefixes, stems, and suffixes.
- Prefixes specify the number of carbon atoms.
- Stems indicate the longest continuous chain of carbon atoms.
- Suffixes indicate the types of bonds (ane, ene, or yne).
- Side groups (substituents) are named and located with regard to the longest chain.
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Description
Test your knowledge on the properties of metals, non-metallic oxides, and ionic compounds. This quiz covers essential concepts in chemistry, including the behavior of metals, types of bonding, and the characteristics of compounds. Perfect for reinforcing your understanding of these foundational topics in chemistry.
