Chapter 4: Chemical Bonding and Molecular Geometry

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30 Terms

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Ionic bonding

attraction between the opposite charges of a cation and an anion, complete transfer of electrons

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Lattice energy

the energy required to completely separate a mole of a solid ionic compound into its gaseous ions

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Coulomb’s Law

force between to particles based on their charge and size

F= k(Q1Q2/r2)

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Covalent bond

bond in which two electrons are shared by two atoms

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Bond enthalpy

change in enthalpy required to break a bond

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Covalent compounds

relatively weak intermolecular forces, liquid, gases, low melting solids

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Ionic compounds

stronger forces, solids with high melting points

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Non-polar covalent bonds

electrons shared equally

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Polar covalent bonds

electrons not shared equally, one atom pulls more

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Electronegativity (EN)

the ability of an atom to attract electrons to itself (determines whether something is polar or non-polar)

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Bond polarity

small EN difference = non-polar covalent

mid EN difference = polar covalent 

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Naming binary molecules

2 non-metal elements in the formula, 2nd element gets “ide” ending, greek prefixes indicate number of atoms

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Naming acids

  1. anions ending in “ide” get hydro prefix, “ic” ending and add “acid” to name

  2. anions ending in “ate” get “ic”, ending in “ite” get “ous” ending

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Naming hydrates

greek prefixes to indicated number of water molecules

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Octet rule

atoms, other than hydrogen, tend to form bonds until surrounded by 8 electrons (have a full octet)

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Formal charge

a way of keeping count of electrons, the charges may or may not be real; the electrical charge difference between valence electrons and the number of electrons assigned to each atom

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Resonance

a better representation of the model of an atom, must be valid lewis structures (occur when you have more than one option of a location to take electrons from)

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Equivalent resonance structures

same formal charge, same number of bond types; low energy (MAJOR) structures contribute more than high energy

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molecular geometry

ignores the lone pairs when naming the structure

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VSEPR

valence shell electron pair repulsion

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Electron domain

region most likely to find electrons in

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Electron geometry

arrangement of electron domains around a central atom 

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non-bonding pairs + repulsion

have greater repulsive forces causes the angles to compress

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multiple bonds + repulsion

exert a great repulsive force on adjacent domains causing the angle to compress

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Diatomic non-polar molecules

same element (H2, O2)

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Diatomic polar molecules

different elements (HCL, CO, NO)

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Polyatomic molecules and polarity

molecular geometry determines if there is a dipole and therefore whether it is polar or non-polar (no net dipole = non-polar, dipole moment = polar)

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Isomer

same formula, different arrangement of atoms

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London dispersion forces

proportional to the number of electrons in the atom

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How to tell if a molecule is polar or non-polar based on the geometry?

polar= overall dipole

non-polar= dipoles cancel out