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Chapter 2: Chemical Compounds and Bonding
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1
Chemical Bonding
The electrostatic attraction between two atoms or ions.
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2
Ionic Bond
A type of bond formed by the complete transfer of electrons from one atom to another.
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3
Covalent Bonding
A type of bonding that involves the sharing of electrons between two atoms.
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4
Valence Electrons
Electrons located in the outermost shell of an atom, important for bonding.
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5
Lewis Structure
A diagram that represents the arrangement of valence electrons in a molecule.
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6
Octet Rule
When atoms combine, they transfer or share electrons so that each atom ends up with 8 electrons in their outermost shell.
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7
Cation
A positively charged ion formed when a metal loses electrons.
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8
Anion
A negatively charged ion formed when a non-metal gains electrons.
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9
Electrostatic Attraction
The force that draws oppositely charged ions together.
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10
Crystal Lattice
The ordered structure in which ionic compounds are arranged in a solid state.
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11
Melting Point
The temperature at which a solid becomes a liquid, affected by ionic bonding strength.
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12
Electrolyte
A substance that conducts electricity when dissolved in water or melted.
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13
Molecular Compound
A compound made up of molecules, typically formed by covalent bonds.
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14
Diatomic Molecule
A molecule that contains two atoms, e.g., H2 or O2.
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15
Triatomic Molecule
A molecule that contains three atoms.
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16
Bonding Capacity
The number of bonds an atom can form based on its valence electrons.
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17
Coordinate Covalent Bond
A bond in which one atom donates both electrons to be shared with another atom.
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18
Intermolecular Forces
Attractions between molecules, including van der Waals forces and hydrogen bonds.
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19
Polar Covalent Bond
A type of bond where electrons are shared unequally, resulting in partial charges.
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20
Electronegativity
A measure of the ability of an atom to attract electrons in a bond.
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21
Ionic Compounds
Compounds formed by ionic bonds, typically consisting of metals and non-metals.
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22
Hydrogen Bonding
A strong type of intermolecular force between hydrogen and highly electronegative atoms.
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23
Lone Pair Electrons
Valence electrons that are not involved in bonding.
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24
Nonpolar Covalent Bond
A bond in which electrons are shared equally, typically between identical atoms.
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25
Melting and Boiling Points of Ionic Compounds
Ionic compounds have high melting and boiling points due to strong ionic bonds.
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26
Dipole
A molecule that has a positive end and a negative end due to electronegativity differences.
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27
Lewis Dot Diagram
A visual representation of an atom's valence electrons using dots.
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28
Isoelectronic
Having the same electron configuration as a noble gas.
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29
Ionization Energy (IE)
The energy required to remove an electron from an atom or ion.
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30
Electron Affinity (EA)
The tendency of an atom to gain or lose electrons.
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31
Chemical Formula
A symbolic representation of a chemical compound indicating the elements and their ratios.
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32
Properties of Covalent Compounds
Varies, can be gases, liquids, or solids with lower melting points than ionic compounds.
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33
Electronegativity Difference
The difference in electronegativity values which determines the type of bond formed.
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34
Van der Waals Forces
Weak attractions between molecules, contributing to the properties of covalent compounds.
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35
HOFBrINCl
An acronym used to remember the diatomic molecules: Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, Chlorine.
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36
Melting Point of Water
0 °C, the temperature at which water transitions from solid to liquid.
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37
High Conductivity
Characteristic of ionic compounds when dissolved in water, allowing for electric current to flow.
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