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AP Chem > 2.1-2.3 > Flashcards

2.1-2.3 Flashcards

1
Q

electronegativity

A

an atom’s ability to attract another atom’s electrons

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2
Q

electronegativity trend

A

increases up (smaller distance to the nucleus) and to the right (smaller radius, more protons)

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3
Q

Coulomb’s law

A

force = k (charges/radius)

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4
Q

attractive force between two particles increases with ______ and decreases with ______.

A

an increase in charge, an increase in the distance

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5
Q

the most electronegative element is…

A

F, fluorine ~ small radius, small shielding

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6
Q

covalent bond

A

between two nonmetals

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7
Q

types of covalent bonds

A

polar and nonpolar

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8
Q

ionic bond

A

between metals and non metals (or polyatomic ions), between cations and anions

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9
Q

nonpolar meaning and number

A

equal share of electrons, less than 0.5

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10
Q

polar meaning and number

A

unequal share of electrons, between 0.5 and 1.7

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11
Q

ionic meaning and number

A

transferred electrons, greater than 1.7

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12
Q

the attraction between positive and negative ions is…

A

a coulombic or electrostatic attraction

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13
Q

metallic bonding

A

between two metal ions (pure or alloys)

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14
Q

alloy

A

a mixture of two or more atoms, at least one of which is a metal

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15
Q

metallic bonds are described as

A

cations in a sea of valence electrons

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16
Q

IMFs are stronger when…

A

there are smaller metallic cations and when there are more valence electrons

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17
Q

metallic character increases…

A

diagonally down

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18
Q

covalent bonds can be…

A

triple, single or double

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19
Q

the more bonds…

A

the more energy needed to break the bonds,
the lesser the distance between atoms

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20
Q

covalent bonds occur at…

A

the lowest energy state, when the attraction between the nuclei is the greatest for the shared electrons, and the repulsions between electrons and between the nuclei is the least, sweet spot at the bottom of the graph

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21
Q

if atoms are too close together the nuclei will…

A

repel each other, top of graph

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22
Q

if atoms are too far apart the attraction…

A

will not be enough to hold them together, far end of graph in middle

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23
Q

bond enthalpy

A

the energy needed to break a bond (absorbed) or form a bond (released)

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24
Q

as radius increases so does

A

bond length

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25
Q

the longer the bond length

A

the lower the bond energy

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26
Q

lattice energy

A

energy needed to separate ions in ionic compounds, combining ions will release energy, represented w/ coulombs law

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27
Q

particle diagrams

A

include clear key with size and element name, include relative size, surround with opposites

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28
Q

properties of ionic compounds

A

form crystals, nonvolatile (slow to vaporize), soluble in polar solvents, high melting and boiling points, hard, brittle, conduct electricity when melted, good insulators when solid, strong

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29
Q

high ion charges

A

stronger bond

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30
Q

larger atoms

A

weaker bonds

31
Q

polarity of the periodic table

A

least polar = closest together, most polar = farthest apart

32
Q

partial negative and positive charges

A

closer to F = partial negative, farther from F = partial positive

33
Q

ionic on the periodic table

A

farther away = more ionic

34
Q

rank from least to most polar: Si-F, S-F, P-F

A

S-F, P-F, Si-F

35
Q

rank from least to most polar: F-F, F-Br, F-Cl

A

F-F, F-Cl, F-Br

36
Q

assign partial negative and positive charges to: H-F

A

H+, F-

37
Q

assign partial negative and positive charges to: S=O

A

S+, O-

38
Q

assign partial negative and positive charges to: P-Cl

A

P+, Cl-

39
Q

Which compound is more ionic? NaF or AgF

A

NaF

40
Q

Which compound is more ionic? BaCl2 or BaS

A

BaCl2

41
Q

Which compound is more ionic? ZnCl2 or SrF2

A

SrF2

42
Q

graph of potential energy and distance

A

shorter bonds more energy (lower)
bigger radius (farther right)

43
Q

colombic attraction in metals

A

number of valence ele determines dumber of electrons in sea, charge of cations and number of ele increase the attractions are greater, when radius decreases so does attraction

44
Q

properties of metals

A

lustrous, malleable, ductile, good conductors of electricity, high BP and MP, strong

45
Q

alloys have

A

the properties of metals

46
Q

interstitial alloys

A

fit in between metal atoms holes

47
Q

substitutional alloys

A

atoms have similar radii, replace atoms in the lattice

48
Q

the ____ electronegative atoms go in the center of a lds

A

least

49
Q

formal charge

A

the charge an atom would have if all of the electrons in a covalent bond were shared equally

50
Q

how to calculate formal charge

A

valence electrons - number of lines and dots

51
Q

best formal charges

A

add up to charge, if neutral all must be zero, central atom has a charge of zero, more electronegative is negative, less electronegative is positive or zero, low

52
Q

fewer than 8 electrons

A

Li, Be, B

53
Q

more than 8 electrons

A

elements in period 3 or below

54
Q

organic compound resonance

A

hexagon with circle or lines

55
Q

localized electrons

A

specifically at one atom or shared between 2

56
Q

delocalized electrons

A

shared by multiple atoms

57
Q

drawing organic molecules

A

connect c, evenly distribute Hs, draw order given

58
Q

element always in center of lds

A

C

59
Q

hybrid orbitals

A

domain counters, when 2 ele domains mix they created 1 less hybridization

60
Q

sigma bonds

A

first bond between two atoms head to head (single, never more than 1)

61
Q

pi bonds

A

side to side overlap

62
Q

bond order

A

the number of bonds shared/the number of atoms

63
Q

if a central atom is symmetrical it is…

A

nonpolar

64
Q

polar molecules

A

have a dipole moment (difference in electronegativity), lone pairs

65
Q

conducting electricity

A

In the solid state, the ions are held by strong coulombic forces in fixed positions within the lattice; thus they cannot move or migrate through the lattice and cannot conduct electricity

66
Q

density in particle diagrams

A

more spread out, less dense

67
Q

metals are both malleable and ductile. The best explanation for these properties is that the electrons involved in bonding among metal atoms are

A

equally shared and form nondirectional bonds

68
Q

one or two total electron domains

A

linear electron domain geometry and molecular domain geometry, bond angle of 180 and sp hybridization for 2 electron domains, nonpolar if no lone pairs

69
Q

3 electron domains

A

trigonal planar
0 unbonded - trigonal planar - 120 - n
1 unbonded - bent - less than 120 - p
2 unbonded - linear - less than 120 - p

70
Q

4 electron domains

A

tetrahedral
0 unbonded - tetrahedral - 109.5 - n
1 un - trigonal pyramidal - <109.5 - p
2 un - bent - <109.5 - p
3 un - linear - <109.5 - p

71
Q

5 electron domains

A

trigonal bipyramidal
0- trigonal bi - 90, 120, 180 - n
1- see saw - 90, <120, 180, p
2- T shaped - 90, 180 - p
3- linear - 180 - n

72
Q

6 electron domains

A

octahedral
0 - octahedral - 90 - n
1 - square pyramidal - 90 - p
2- square planar - 90 n

73
Q

5 and 6 domains hybridization

A

sp3d, sp3d2

AP Chem (10 decks)

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