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Chemistry > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Convert kg to g

convert mg to g
3mg convert to grams

A
  1. 1 kg is = to 1000 g

2. g times 10 to the negative 3

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2
Q

Electronegativity __________ across a period

and _____________ down a column

A

increases

decreases

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3
Q

A _______ electronegativity difference leads to a higher bond polarity. A ________ electronegativity difference leads to a lower bond polarity

A

higher

lower

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4
Q

What is a dipole moment

A

it occurs anytime there is a separation of positive and negative charge

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5
Q

As bond order __________ the bond gets stronger (Greater bond energy)
and that results in __________ (shorter or longer) bond lengths

A

increases

shorter

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6
Q

bonding between a metal and nonmetal

bonding between a nonmetal and nonmetal

A

ionic bonding

covalent bonding

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7
Q

In the band theory, what do you call the molecular orbitals that are occupied

what do you call the orbitals that are unoccupied

A

valence band = occupied

conduction band = unoccupied

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8
Q

When there is no energy gap between the conduction band and valence band what does that mean

When there is a small energy gap between the conduction band and valence band

When there is a large energy gap between the conduction band and valence band what does that mean

A

conductor

semiconductor

insulator

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9
Q

What is a molecular compound

A

2 or more nonmetals = covalent bond only

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10
Q

What are the rules for naming a molecular compound

A
  1. identify it as a molecular compound
  2. write name of element with smallest group number first
  3. If the two elements lie in the same group, write element with greatest row number first
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11
Q

What is the form for writing a molecular compound name

A

prefix (if needed) - Name of first element (smallest group #) - prefix of second element - base name of second element plus -ide

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12
Q

What is the name of NO2

N20?

NI3

A
  1. Nitrogen dioxide
  2. dinitrogen monoxide
  3. Nitrogen triiodide
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13
Q

Write formula for Phosphorus tribromide

A

PBr3

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14
Q

what is the atomic mass?

A

average mass of atom

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15
Q

What is the formula mass

what is it also called?

A

average mass of molecule of a compound

molecular mass or molecular weight

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16
Q

How do you get formula mass?

A

[(number of atoms of 1st element in chem formula) times (atomic mass of first element)] + [(number of atoms of 2nd element in formula) times (atomic mass of first element)] etc….

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17
Q

What is the formula mass for CO2

A

C= 12.01 0=16

Formula mass= 12.01+ (2*16)= 44.01

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18
Q

What is the molar mass of a compound

A

mass in grams of one mol of its molecules or formula units - numerically equivalent to its formula mass 5.9

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19
Q

Find number of CO2 molcules in a sample of dry ice (solid CO2) with mass of 10.8 g

A

Plan:
grams CO2 to moles of CO2 to CO2 moledcules (remember to use the avogardo number when converting to molecules)

should get 1.48 times 10 to the 23 CO2 molecules

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20
Q

what do you use avogardo number for

A

for converting any compound of moles to molecules

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21
Q

What is mass percent

how do you find it

A

mass %= percent of compounds total mass

find it by
mass% of element x within a given compound = mass of element x in one mol of compound divided by mass of 1 mol of compound

22
Q

CCl2F2 calc mass % of Cl

A

mass % Cl=

first find molar mass of whole thing
than take Cl molar mass divided by entire molar massthen times by 100=
58.64%

23
Q

what are organic compounds composed of

A

carbon and hydrogen

24
Q

What is the key element in organic compounds

A

Carbon because always form four bonds

25
Q

organic vs inorganic

A 
organ= living 
in= originate from earth
26
Q

what are hydrocarbons

A

simpelest organic compounds / composed of hydrogen and carbon

27
Q

does a pair of electrons have to be shared equally amongst compound

A

no unequal results in polar covalent bonds

28
Q

what is electronegativity

A

ability of an atom to attract electrons to itself in a chem bond (results in polar and ionic bonds)

29
Q

what does polar covalent mean

A

there is an intermediate electronegative difference between the two atoms (one has more of electron than other)

30
Q

What is purely covalent

A

bond where electrons are equally shared

31
Q

what is a dipole moment

A

occurs anytime there is a seperationof positive and negative charge

32
Q

what is percent ionic character

A

ratio of bond’s actual dipole moment to the dipole moment it would have if the electron were completely transferred from one atom to the other times 100

33
Q

The smaller the magnitude of the charge separation and the smaller the distance between the charges, the smaller the dipole moment

A

true

34
Q

if an electron is completely transferred from one atom to another what would the % ionic character be

A

100%

35
Q

percent ionic character _____________ (inc. or dec.) as the electronegativity difference ________ (inc. or dec.)

A

inc.

inc

36
Q

what is the bond energy

A

of a chem bond it is the energy required to break one mole of the bond in the gas phase

37
Q

what are the 5 basic shapes according to the number of electron groups surrounding a central atom and their bond angles

A
  1. linear (2) …180
  2. trigonal planar (3). 120
  3. tetrahedral (4)… 109.5
  4. trigonal bipyrimidal (5)….. 120/90
  5. octahedral (6)…. 90
38
Q

When a triangular (trigonal ) planar has one lone pair and two bonded pairs what molecular geo does it take on

A

eg= triangular planar mg= bent or angular

39
Q

Tetrahedral molecular geo when one lone pair

two lone pairs

A

one= triangular pyramidal

two= bent or angular

40
Q

triangular bipyrimidal one lone pair

two lone pairs

three lone pairs

A

one= see saw

two= t shaped

three= linear

41
Q

octahedron with one lone pair

two lone pairs

A 
one= square pyramidal
two= square planar
42
Q

what are magnetic properties a result of

A

due to electrons

unpaired elecrons cause magnetism

43
Q

what is the flaw in the lewis structure

A

does not predict magnetic properties

44
Q

what is the valence bond theory

A

a chem bond is overlap between two half filled atomic orbitals

45
Q

______________ (higher or lower) bond order= ____________ (weaker or stronger) bond

A

higher

stronger

46
Q

what is the formula for bond order

A

of electrons in bonding Molecular oribitals - number of electrons in antibonding molecular orbitals all divded by two

47
Q

if 1 or higher than compound is considered stable?

A

true

48
Q

what is earth’s most significant greenhouse gas

A

cabon dioxide

49
Q

what does CO2 doe to the atmosphere

A

enhances ability to hold heat = global warming

50
Q

chem change vs physical change

A 
chem= atoms rearrange 
ex= rusting iron, burning sugar, transformation of oxygen and CO2 to glucose

phys= no change in arrangement
ex boiling water, changing state of matter, physically crushing something

51
Q

what are some guidelines for balancing equations

A

start withmost complex comound first

and to clear fraction times by denominator to everything in reactant

52
Q

stoichiometry analougy is what

A

recipies ex pizza

Chemistry (7 decks)

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