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CHEMISTRY unit 1 > chapter 2 > Flashcards

chapter 2 Flashcards

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1
Q

what does a lewis structure show ?

A

the arrangement of electrons and bonds in a molecule or polyatomic ion

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2
Q

if the difference of EN > 1.7

A

ionic

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3
Q

if the difference of EN < 1.7 > 0.5

A

polar covalent

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4
Q

if the difference of EN < 0.5

A

non-polar covalent

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5
Q

in ionic bonds, the valence electrons are

A

transferred

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6
Q

in polar covalent bonds, the valence electrons are

A

shared unequally (partial charges)

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7
Q

in non polar covalent bonds, the valence electrons are

A

shared equally

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8
Q

what are ions formed and held together by ?

A

electrostatic attraction

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9
Q

atoms and ions are stable if they have

A

a full valence shell of electrons

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10
Q

electrons are most stable when

A

paired

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11
Q

atoms form chemical bonds to

A

achieve a full valence shell

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12
Q

a full valence shell may be achieved by either

A

transferring or sharing electrons

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13
Q

what are the 3 types of ionic compounds ?

A

binary ionic compounds
polyatomic ionic compounds
ionic compounds with multivalent metals

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14
Q

binary ionic compounds (how many ? what do they end in ?)

A

2 elements: 1 metal and 1 non-metal

end in -ide

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15
Q

polyatomic compounds (how many ? what do they end in ?)

A

more than 2 elements: 1 metal and 1 polyatomic ion

compound names usually end in -ate or -ite

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16
Q

compounds with multivalent metals

A

contain a metal with more than one possible charge

roman numerals indicate charge

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17
Q

which compounds use roman numerals to indicate charge ?

A

multivalent metals

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18
Q

what kind of compounds do NOT criss cross charges ?

A

molecular/covalent compounds

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19
Q

covalent/molecular compounds contain, end in ?

A

contain 2 or more non-metals

end in -ide

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20
Q

what kind of compounds use prefixes ?

A

molecular/covalent

hydrates

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21
Q

list the prefixes

A 
mono
di
tri
tetra
penta
hexa
hepta
octo
nona
deca
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22
Q

what are the two types of acids ?

A

binary acids

oxy acids

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23
Q

what are binary acids composed of ?

A

H and one other element

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24
Q

what are oxy acids composed of ?

A

H and a polyatomic ion

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25
Q

all acids are

A

aq

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26
Q

what kind of acids start with hydro-

A

binary acids

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27
Q

give an example of a binary acid

A

hydrochloric acid

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28
Q

binary acids end in

A

-ic

29
Q

when writing acids, for polyatomic ions that end in -ate, the acid ends in

A

-ic

30
Q

when writing acids, for polyatomic ions that end in -ite, the acid ends in

A

-ous

31
Q

what does VSEPR stand for ?

A

valence shell electron pair repulsion

32
Q

who developed the VSEPR theory ?

A

Ronald Gillespie and Ronald Nyholm

33
Q

what is the VSEPR theory ?

A

a model for predicting the shape of molecules

34
Q

what is important for molecular shape ?

A

the valence shell electrons of the central atoms

35
Q

what do valence shell electron pairs do ?

A

they repel each other electrostatically

36
Q

what determines the molecular shape ?

A

the positions of the electron pairs when they are a maximum distance apart (with the lowest repulsion possible)

37
Q

what do geometrical arrangements refer to ?

A

refers to the ways in which the groups of valence electrons are positioned around the central atom

38
Q

how many basic geometrical arrangements and what do they result from ?

A

there are 5 basic geometrical arrangements

result from the interactions of lone pairs and bonding of electrons

39
Q

list the 5 basic geometrical arrangements ?

A 
linear
trigonal planar
tetrahedral
trigonal bipyramidal
octahedral
40
Q

variations in the molecular shape occur if

A

one or more of the electron groups include a lone pair of electrons

41
Q

2 bonds (0 lp) = 2

A

linear

42
Q

3 bonds (0 lp) = 3

A

trigonal planar

43
Q

4 bonds (0 lp) = 4

A

tetrahedral

44
Q

5 bonds (0 lp) = 5

A

trigonal bipyramidal

45
Q

6 bonds (0 lp) = 6

A

octahedral

46
Q

2 bonds 1 lp = 3

A

bent

47
Q

3 bonds 1 lp = 4

A

trigonal pyramidal

48
Q

2 bonds 2 lp = 4

A

bent

49
Q

4 bonds 1 lp = 5

A

sawhorse

50
Q

3 bonds 2 lp = 5

A

t-shaped

51
Q

2 bonds 3 lp = 5

A

linear

52
Q

5 bonds 1 lp = 6

A

square pyramidal

53
Q

4 bonds 2 lp = 6

A

square planar

54
Q

overall polarity of a molecule depends on

A 
dipole moments (location of partial charges)
molecular shape
55
Q

in order for a molecule to be POLAR, it must have..

A

polar covalent bonds

nonsymmetrical partial charge distribution

56
Q

what determines the melting and boiling points of a compound ?

A

the strength of the force between ions or molecules

57
Q

____ compounds usually have HIGH mp and bp

A

ionic

58
Q

____ compounds have intermediate mps and bps

A

polar covalent

59
Q

____ molecules have the lowest mp and bp

A

non polar covalent

60
Q

water is a _____ molecule

A

polar

61
Q

what kind of compounds are insoluble in water ?

A

non polar covalent compounds

62
Q

what kind of compounds are soluble in water ?

A

ionic and polar covalent

63
Q

in order to conduct an electric current, ions must

A

be free to move

64
Q

which state of ionic compounds can conduct electricity ?

A

liquid and aqueous

65
Q

what are INTERmolecular forces ?

A

attractions between molecules

66
Q

what are INTRAmolecular forces ?

A

forces within molecules

67
Q

which forces are stronger, intermolecular or intramolecular ?

A

intramolecular forces are stronger

68
Q

intermolecular forces as a group are referred to as

A

van der waals forces

CHEMISTRY unit 1 (3 decks)

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