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College Chemistry (Gen, Organic, BioChem) > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

Electrons are what cause

A

chemical reactions

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2
Q

electrons can be found in

A

different energy levels

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3
Q

each energy level corresponds to a

A

row on the periodic table

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4
Q

Horizontal rows of elements = X = X

A

period = no. of occupied e- shells

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5
Q

each energy level has what

A

sub-levels

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6
Q

electrons fill from

A

right to left

top to bottom

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7
Q

1S^1 what does each stand for

A 
1= energy level
S= sub level
^1= # of electron in the orbital
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8
Q

box diagrams

A

look at college or high school notes

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9
Q

valence electrons

how many does each group have

A

electrons in the highest energy level

g1= 1, g2=2, g3=3, g4=4, g5=5, g6=6, g7=7, g8=8

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10
Q

just as protons increase across the periodic table, what also increases

A

electrons

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11
Q

noble gases have how many valence electrons

A

8

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12
Q

the octet rule ?

A

atoms are most stable when they have 8 electrons in their valence shell

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13
Q

valence electrons are the

A

outermost, highest energy electrons

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14
Q

exceptions of the octet rule

A

H and He

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15
Q

noble gases all have

A

8 valence electrons

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16
Q

why are noble gases some of the last elements to be discovered

A

because they do not readily react

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17
Q

octet rule cont. – Atoms will

A

gain or lose electrons to have 8 valence electrons

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18
Q

atoms will gain or lose electrons to form

A

ions

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19
Q

what are the types of ions

A

cations and anions

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20
Q

what are cations

A

when a neutral atom has a loss of an electron

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21
Q

what are anions

A

when a neutral atom has a gain of an electron

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22
Q

Ca2+ has what biological important

A

1.5-2% of body mass, bones, teeth

necessary for blood clotting, digestion, formation of bones and teeth, actions of muscle(heart)

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23
Q

Mg2+ has what biological important

A

bones and teeth, intracellular activity

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24
Q

Fe2+ has what biological Important

A

neccessary for formation of hemoglobin and cytochromes, O2 transfer

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25
Q

Cu2+ has what biological important

A

cofactor in enzymes

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26
Q

Zn2+ has what biological important

A

cofactor in enzymes, growth, healing

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27
Q

Co3+ has what biological important

A

in vitamin B12

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28
Q

Na+ and K+ has what biological important

A

water balance, nerve impulses, fluids inside and outside cells
Na+= extracellular positive ion
K+ Intracellular positive ion

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29
Q

cations ??

A

lose electrons

become more positive

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30
Q

cation elements are written

A

with symbol and a #+ or +# to the upper right

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31
Q

In Cations you must indicate

A

how many electrons have been lost

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32
Q

cations are named

A

as “element name and ion”

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33
Q

some metals can lose different

A

of electrons

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34
Q

transition metals, you must include

A

charger

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35
Q

ions, some metals

A

can lose different # of electrons

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36
Q

Anions ??

A

gain electrons

they become more negative

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37
Q

which nonmetals will become anions

A

nonmetals in groups 5,6,7

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38
Q

which metals will become cations

A

metals in groups 1,2,3

group 4 is iffy

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39
Q

in anions, you must indicate

A

how many electrons have been gained

40
Q

Anions are named

A

as “element name ending in -ide and ion”

41
Q

prediction Ion charges?? what are they

A 
G1= 1+
G2=2+
G3=3+
G4=4+-
G5=3-
G6=2-
G7=1-
G8=0
42
Q

polyatomic ions

A

sometimes groups of atoms bounded together will have a overall net charge

43
Q

what does it mean to be an isoelectronic atom

A

they have the same electron configuration

44
Q

during lewis dot structures, valence electrons

A

can be depicted as dots around the element symbol

45
Q

lewis dot structures can be used to

A

predict bonding behavior in atoms

46
Q

what are the 3 types of bond

A

ionic bond, polar covalent, and nonpolar covalent

47
Q

what are ionic bonds

A

give and take electrons

metals with nonmetals

48
Q

what are nonpolar covalent bonds

A

nonmetals with nonmetals

share electrons equally

49
Q

what are polar covalent bonds

A

nonmetal with nonmetal

share electrons but not equally

50
Q

why do nonmetals have high electronegativty

A

nonmetals are negative and pull electrons towards them which means high electronegativity

51
Q

what is the electronegative difference for pure covalent

A

<0.4

52
Q

what is the electronegative difference for polar covalent

A

between 0.4 & 1.8

53
Q

what is the electronegativity difference for ionic bond

A

> 1.8

54
Q

how do elements combine

A

atoms can donate or accept valence electrons to reach 8 VE-

atoms will bond together this way forming ionic bonds

55
Q

naming ionic compounds found in S or P orbitals

A

write the periodic table name for the cation
write the name of the anion 2nd, but change the last 3 letters of the anions name to “ide”
DO NOT WRITE ANY NUMBERS WITH THE NAMES

56
Q

naming ionic compounds found in D orbitals

A

write the periodic table name for the cation
after the cation is written, write the roman numeral for the ion’s charge in partentheses
write the anion 2nd and change the ending to “ide”
NO OTHER NUMBERS NEEDED

57
Q

Naming with polyatomic ions

A

write the periodic name for the cation(make sure if D orbital roman numeral is there)
write the anion 2nd, no changes to name –write it how it is on the polyatomic ion sheet
IF THE 2ND ION IS ON THE PERIODC TABLE, CHANGE THE ENDING TO “IDE”

58
Q

Writing ionic compounds

A

total charges need to= total-charges
or + and - need to add up to 0
number of each element is included as a subscript
cation 1st, anion 2nd

59
Q

On the polyatomic ion sheet, most of them have what in it

A

oxygen (known as oxyanions)

60
Q

writing ionic compounds w/polyatomic ions

A

write the cations name, no changes to name 1st

name anion 2nd - use polyatomic name

61
Q

in covalent bonds, no what are formed?

A

no ions are formed=no charges to balance

62
Q

writing covalent compounds

A

element farthest to the left is written first
elements to the right are written 2nd, 3rd, 4th, etc.
subscripts are used to indicate how many of each element are present
last element name ends in “IDE”

63
Q

naming covalent compounds - numerial prefixes

A 
mono-1
di-2
tri-3
tetra-4
penta-5
hexa-6
hepta-7
octa-8
nana-9
deca-10
last element name ends in "IDE"
64
Q

a mol in chemistry is

A

a way of quantifying or counting atoms & molecules

65
Q

a mol relates

A

the mass of elements to numbers of atoms it contains

66
Q

how do we count atoms and molecules in moles

A

by avogrado’s number

67
Q

what is avagadros number

A

6.02 X 10^23

68
Q

One mol of an element is equal to what

A

equal to its atomic mass in grams

69
Q

one mol of a compound is equal to what

A

equal to the sum of its atom’s atomic masses in grams

70
Q

for mole coversions, we only need to know what 2 things

A

molar mass and avagadros #

71
Q

mass cannot be

A

created or destroyed

72
Q

the coeffiants represent what in a balanced equation

A

represent mole ratios

73
Q

mole ratios can be used to convert to

A

mass or molecules

74
Q

mole conversions steps

A

balance equation
find molar mass of what you have
find molar mass of what you need
use coefficants and dimensional analysis to solve

75
Q

not all covalent bonds are created

A

equal

76
Q

chemical bonding are used in

A

correct dosages
dru g interactions
how compounds react with the body, cells, tissues and organs

77
Q

some(most) covalent bonds include

A

unequal sharing of electrons

78
Q

electronegatvity def

A

the ability to attract electrons

79
Q

as you go from left to right, your electronegativity

as you go from bottom to top, your elecrtonegativity

A

L to R = increase

bottom to top=increases

80
Q

polar covalent bonds

A

unequal distribution of electrons

81
Q

dipole movement

A

dipole movement has a magnitude and a direction

82
Q

nonpolar covalent bonds

A

equal distribution of electrons

83
Q

determining polarity step 1.

A

1) is the molecule a hydrocarbon?
no- determine the molecules lewis structure
yes- molecule nonpolar

84
Q

determining polarity step 2.

A

2) determining the molecules shape

85
Q

determining polarity step 3.

A

3) is my shape symmetric
no- molecule polar
yes- examine outside atoms

86
Q

determing polarity step 4.

A

4) if the shape is symmetric, are all outside atoms the same
no-molecule polar
yes-molecule is nonpolr

87
Q

the polarity is due to the

A

lone pair on the central oxygen atom

88
Q

what is molecular geometry

A

electrons are negatively charged
they repel eachother
electron orbitals repel eachother

89
Q

it is the outermost or valence electrons that interact

A

NEED TO KNOW

90
Q

think of atoms like balloons– they pull??

A

eachother apart at maximum angles

91
Q

we use lewis dot diagrams to

A

represent valance electrons to predict the shape of molecules

92
Q

what does VSEPR stand for

A

valence shell electron pair repulsion

93
Q

what is the VSEPR theory

A

predicts geometry of molecules based on electron repulsions

94
Q

each pair of electron pair counts as

A

one electron domain

95
Q

double and triple bonds count as

A

one electron domain

College Chemistry (Gen, Organic, BioChem) (3 decks)

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