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General Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

lewis dos structure

A
  • type of model used to represent what compounds look like at the molecular level
  • helps understand the elements reactivity
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2
Q

single bond

A

a bond formed from two electrons

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3
Q

double bonds

A

use four electrons

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4
Q

triple bonds

A

use six electrons

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5
Q

Resonance structures are two or more structures where

A

only nonbonding electrons, and double and triple bonds may move around

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6
Q

bond dissociation energy (BDE)

A

the energy required to break a bond homolytically

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7
Q

homolytic bond cleavage

A
  • one electron of the bond being broken goes to each fragment of the molecule
  • two radicals form
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8
Q

heterolytic bond cleavage

A
  • also known as dissociation
  • both electrons of the electron pair that make up the bond end up on the same atom
  • forms both a cation and an anion
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9
Q

bond order

A

the number of bonds between adjacent atoms, so a single bond has a bond order of 1 while a triple bond has a bond order of 3

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10
Q

the longer the bond, the ______ it is

the shorter the bond, the ______ it is

A
  1. weaker

2. stronger

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11
Q

covalent bond

A
  • formed between atoms when each contributes one or more of its unpaired valence electrons
  • electrons are shared by both atoms to help complete both octets
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12
Q

electronegativity

A

atom’s ability to attract another atom’s valence electrons when it forms a bond

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13
Q

when and why is a bond polar?

A
  • when the electron density between the two nuclei is uneven
  • occurs if there is a difference in electronegativity of the bonding atoms, the greater the difference, the more uneven the electron density and the greater the dipole moment
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14
Q

when and why is a bond nonpolar?

A
  • when the electron density between to nuclei is even
  • occurs when there is little to no difference in electronegativity between the bonded atoms
  • generally happens when two atoms of the same element are bonded to each other
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15
Q

coordinate covalent bond

A

when an atom donates both of the shared electrons in a bond

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16
Q

when a coordinate covalent bond breaks, the electrons that come form the _______ will leave with that ______.

A
  1. ligand (nucleophile)

2. ligand

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17
Q

lewis base / ligand

A

a molecule or ion that donates a pair of nonbonding electrons

18
Q

ionic bond

A

bond between a cation and an anion

19
Q

ionic bond strength

A

is proportional to the charges on the ions, it decreases as the ions get farther apart, or as the ionic radii increase

20
Q

valence shell electron-pair repulsion theroy (VSEPR)

A

since electrons repel one another, electron pairs, whether bonding or nonbonding, attempt to move as fas as possible

21
Q

orbital geometry

A

determined by the total number of electron groups on the central atom of a molecule

22
Q

hybridization of H2O

A

sp3 (tetrahedral)

23
Q

hybridization of SO2

A

sp2 (trigonal planar)

24
Q

hybridization of NH4

A

sp3 (tetrahedral)

25
Q

hybridization PCL3

A

sp3 (tetrahedral)

26
Q

hybridization of CO3^2-

A

sp2 (trigonal planar)

27
Q

sigma bond

A

consists of two electrons that are localized between two nuclei
formed by the end-to-end overlap of one hybridized orbital from each of the two atoms participating in the bond

28
Q

pi (π) bond

A

composed of two electrons that are localized to the region that lies on opposite sides of the plane formed by the two bonded nuclei and immediately adjacent atoms, not directly between the two nuclei as with the sigma bond

29
Q

intermolecular forces

A

the relatively weak interactions that take place between neutral molecules

30
Q

dipole-dipole interactions

A

the attractions between the positive end of one polar molecule and the negative end of another polar molecule

31
Q

dipole-induced dipole force

A

happens when a permanent dipole in one molecule may induce a dipole in a neighboring nonpolar molecule

32
Q

london dispersion forces

A

very weak and transient interactions between the instantaneous dipoles in nonpolar molecules

33
Q

ion-dipole

A

polar molecules attracted to ions

34
Q

hydrogen bonding

A

strongest type of intermolecular force between neutral molecules

35
Q

requirements for hydrogen bonding

A
  1. a molecule must have a covalent bond between H and either FON
  2. another molecule must have a lone pair of electrons on an N, O, F atom
    ex: water
36
Q

vapor pressure

A
  • physical property determined by the strength of the intermolecular forces of a substance
  • pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid
  • the weaker a substance’s intermolecular forces, the higher its vapor pressure and the more easily it evaporates
  • it is temperature dependent, it increases with the temperature of the substance
37
Q

ionic solids

A
  • held together by the electrostatic attraction between cations and anions in a lattice structure
  • strong
  • most of this ionic substances are solid at room temperature
  • the greater the charge, the stronger the force of attraction between the ions
  • the smaller the ions, the more they are attracted to each other
38
Q

network solids

A
  • atoms are connected in a lattice of covalent bonds, all interactions between atoms are covalent bonds
  • the intermolecular forces are identical to the intramolecular forces
  • very strong
  • tend to be very hard solids at room temperature
  • ex: diamond and quartz
39
Q

metallic solids

A
  • metals are excellent conductors of electricity and heat, are malleable and ductile
  • vary widely in strength
  • almost all metals are solid at room temperature
40
Q

molecular solids

A
  • held together by one of three types of intermolecular interactions: hydrogen bonds, dipole-dipole forces or London dispersion forces
  • typically have much lower melting and boiling points than the other types of solid
  • often liquids or gases at room temp
  • tend to be solids as the strength of their intermolecular forces increases

General Chemistry (2 decks)

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