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Chemistry Test 1-chapter 1 and 2 > chapters 3 and 4 > Flashcards

chapters 3 and 4 Flashcards

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1
Q

ionic bonding

A

the complete transfer of valence electrons

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2
Q

covalent bonding

A

sharing of electrons

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3
Q

polar bonds

A

unequal sharing of electrons

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4
Q

general trend of electronegativity

A

increases going left to right and up a column

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5
Q

VSEPR theory

A

structures surrounding and atom is determined by minimizing electron pair repulsions

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6
Q

chemical bond

A

force that holds atoms together

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7
Q

bond energy

A

required energy to break a bond

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8
Q

bond length

A

distance where energy is minimal

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9
Q

nonmetallic elements achieve a noble gas configuration by _____ electrons

A

sharing

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10
Q

metals are _____

A

cations

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11
Q

nonmetals are _____

A

anions

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12
Q

cation is generally _____ than parent atom

A

smaller

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13
Q

anions are generally _____ than parent atom

A

larger

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14
Q

ion size______ going down a group

A

increases

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15
Q

ions generally adapt ______ configurations in ionic compounds

A

noble gas electron

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16
Q

isoelectronic ions

A

ions containing the same number of electrons

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17
Q

______ protons means ______ attraction and _______ ions

A

more, greater, smaller

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18
Q

electronegativity

A

ability of an electron to attract shared electrons to itself

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19
Q

lattice energy

A

change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

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20
Q

all compounds with _____% or more ionic character are considered to be ionic solids

A

50

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21
Q

delocalization of electrons

A

eletrons free to move through entire molecule

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22
Q

as number of shared electrons _____ bond length _____

A

increases, shortens

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23
Q

energy terms with bond breaking have a ____ sign

A

positive

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24
Q

energy terms with bond making have a ___ sign

A

negative

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25
Q

list the exceptions to the octet rule

A

boron, and any row 3 or lower

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26
Q

resonance

A

when more than one correct lewis structure can be drawn

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27
Q

formal charge formula

A

valence-non bonding-bonding/2

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28
Q

valence electron formula

A

lone pairs+ 1/2(shared electrons)

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29
Q

how to name type 1 compounds

A

cation first anion 2nd
cation takes name from element
anion named by taking root of element name and adding -ide

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30
Q

how to name type 2 compounds

A

same as type one
cation first then anion
must specify the charge
add -ide to the end

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31
Q

how to name type 3 compounds

A

first element named with full name
2nd element named like anion
prefixes for the nunber of atoms
mono prefix not used for first element

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32
Q

molecular structure

A

3d arrangement of atoms in a molecule

33
Q

2 pairs of electrons means what shape

A

linear

34
Q

3 pairs of electrons means what shape

A

trigonal planar

35
Q

4 pairs of electrons means what shape

A

tetrahedral

36
Q

5 pairs of electrons means what shape

A

trigonal bipyramidal

37
Q

6 pairs of electrons means what shape

A

octahedral

38
Q

true or false in vsper a double bond is counted as one effective pair

A

true

39
Q

dipole moment

A

molecule with a center of positive and negative charge

40
Q

electrostatic potential diagram

A

colors of visible light are used to show the variation in charge distribution
red= electron rich
blue= electron poor

41
Q

hybridization

A

mixing of native atomic orbitals to form special orbitals for bonding

42
Q

sigma bond

A

electron pair is shared in an area centered on a line running in between the atoms

43
Q

pi bond

A

parallel p orbitals that occupy space above and belowine joining atoms

44
Q

in a single bond how many sigma bonds are there

A

1

45
Q

in a double bond there is ____ sigma and ____pi

A

1 and 1

46
Q

in a triple bond there is ____ sigma and ___pi

A

1 and 2

47
Q

bond order

A

(bonding electons-antibonding electrons)/2

48
Q

_____ bond order means ____bond strength

A

larger, greater

49
Q

paramagnetic

A

unpaired electrons make something paramagnetic

50
Q

diamagnetic

A

when all electrons are paired

51
Q

as bond order _____ bond energy _____ and bond length _____

A

increases, increases, decreases

52
Q

is o2 paramagnetic or diamagnetic

A

paramagnetic

53
Q

electron geometry

A

includes lone pairs and bonding electrons

54
Q

molecular geometry

A

includes only bonding pairs

55
Q

nonpolar

A

if molecule has a symmetric shape and like bonds

56
Q

formal for change in E

A

change in E=bonds broken-bonds formed

57
Q

ionic bonds generally form between what

A

metals and nonmetals

58
Q

to choose best lewis structure using formal charge the charge of the central atoms should be close to ____

A

zero

59
Q

what shape has sp hybridization

A

linear

60
Q

what shapes have sp2 hybridization

A

bent and trigonal planar

61
Q

what shapes have sp3 hybridization

A

tetrahedral, seesaw, trigonal pyramidal

62
Q

what shapes have sp3d hybridization

A

trigonal bipyramidal

63
Q

what shape has sp3d2 hybridization

A

octahedral

64
Q

ammonium

A

NH4+

65
Q

carbonate

A

CO3^2-

66
Q

chlorate

A

ClO3-

67
Q

chromate

A

CrO4^2-

68
Q

cyanide

A

CN-

69
Q

hydroxide

A

OH-

70
Q

nitrate

A

NO3-

71
Q

phosphate

A

PO4^3-

72
Q

sulfate

A

SO4^2-

73
Q

permanganate

A

MnO4-

74
Q

type 2 compounds typically involve….

A

transition metals

75
Q

type 3 compounds are made of…

A

two nonmetals

76
Q

type 1 compounds always have…

A

a cation and anion

77
Q

single bond has a bond order of

A

1

78
Q

double bond has a bond order of 2

A

triple bond has a bond order of 3

Chemistry Test 1-chapter 1 and 2 (4 decks)

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