Exam 1 Review

Question 1

matter

Answer 1

that which has mass and volume

Question 2

law of conservation of mass

Answer 2

mass is neither created or destroyed in a normal chemical rxn

Question 3

law of definite proportions

Answer 3

all samples of a pure compound have the same proportions by mass of their constituent elements

Question 4

law of multiple proportions

Answer 4

when atoms of 2 elements combine to make 2 different compounds, the mass of the element A that combine with B in the 2 can be expressed as a ratio of small whole numbers

Question 5

extensive property

Answer 5

depends on amount

Question 6

intensive property

Answer 6

independent of amount

Question 7

femto (f)

Answer 7

10^-15

Question 8

pico(p)

Answer 8

10^-12

Question 9

nano(n)

Answer 9

10^-9

Question 10

micro(u)

Answer 10

10^-6

Question 11

milli(m)

Answer 11

10^3

Question 12

centi(c)

Answer 12

10^-2

Question 13

deci(d)

Answer 13

10^-1

Question 14

kilo(k)

Answer 14

10^3

Question 15

mega(M)

Answer 15

10^6

Question 16

giga(G)

Answer 16

10^9

Question 17

tera(T)

Answer 17

10^12

Question 18

Cathode ray experiment

Answer 18

discovers electron, negative charge, and charge to mass ratio

Question 19

Oil drop experiment

Answer 19

measured the strength of E-field necessary to halt the free fall oil droplets deducing the charge of an electron and thus the mass

Question 20

Gold foil experiment

Answer 20

alpha particles passed through gold foil, most went straight though, some deflected, evidence for nuclear theory of the atom

Question 21

nuclear theory of the atom

Answer 21

-most of atom’s mass and all its positive charge are in a dense region called nucleus

Question 22

frequency equation

Answer 22

f=c/wavelength

Question 23

KE of ejected electron

Answer 23

Ephoton - Ebinding

Question 24

Ephoton

Answer 24

hf

Question 25

de broglie wavelength

Answer 25

a moving e- has a wavelength = h/mv

Question 26

Heinsberg Uncertainty

Answer 26

we cannot simultaneously observe the wave and particle nature of electrons, the act of observation forced the electron into one state or another. (uncertainty in position)(m*uncertainty in velocity) >= h/4pi

Question 27

indeterminancy

Answer 27

the present doe not determine the future; one can only know probability of finding electron in a certain region

Question 28

principle quantum number (n)

Answer 28

overall size and energy level of an orbital, n=1,2,3,...

Question 29

angular momentum quantum number (l)

Answer 29

determines the shape of the orbital, l=0...(n-1).

Question 30

l=0

Answer 30

s

Question 31

l=1

Answer 31

p

Question 32

l=2

Answer 32

d

Question 33

l=3

Answer 33

f

Question 34

magnetic quantum number(ml)

Answer 34

specifies orientation of orbital, ml = -l to +l (integers)

Question 35

spin quantum number (ms)

Answer 35

ms= -1/2 or +1/2

Question 36

group 1a

Answer 36

alkali earth metals

Question 37

group 2a

Answer 37

alkaline earth metals

Question 38

group 7a

Answer 38

halogens

Question 39

group 8a

Answer 39

noble gases

Question 40

pauli exclusion principle

Answer 40

no 2 electrons in an atom can have the same 4 quantum numbers

Question 41

aufbau principle

Answer 41

lowest energy orbitals are filled first

Question 42

hunds rule

Answer 42

electrons first fill singly with II spins, then they pair

Question 43

metals

Answer 43

tend to lose e, good conductors of heat and electricity, malleable, ductile

Question 44

nonmetals

Answer 44

tend to gain electrons, poor conductors

Question 45

metalloids

Answer 45

semiconductors

Question 46

atomic radius

Answer 46

increases down a group bc n increases resulting in larger orbitals, decreases across a period bc Zeff increases. remains roughly constant in transition elements bc outermost principle energy level remain constant after 1st 2 groups of transition

Question 47

transition cations

Answer 47

ns electrons removed before (n-1)d

Question 48

paramagnetic

Answer 48

an atom that contains one or more unpaired electrons is attracted to external magnetic field

Question 49

diamagnetic

Answer 49

an atom with all electrons paired is slightly repelled by external magnetic field. proof of how transition cations are formed

Question 50

ionic radii

Answer 50

cations are smaller than original element, anions are larger

Question 51

ionization energy

Answer 51

energy required to remove an electron; 1st ie decreases down a group, increases across a period . successive ionization energies - increase, then really increase once noble gas config is reached

Question 52

exceptions to ie trends

Answer 52

when going from s to p orbital, half filled shell (N and O)

Question 53

electron affinity

Answer 53

energy change associated with the gaining of an electron; only 1a has a group trend, becomes more positive. across period ea becomes more negative (adding electron would release more energy into the atmosphere)

Question 54

chemical bonds

Answer 54

form bc they lower pe of charged particles that compose atoms

Question 55

ionic bond

Answer 55

btwn metal and nonmetal, transfer of electrons, forms a lattice of alternating cations and anions

Question 56

covalent compounds

Answer 56

2 or more nonmetals, share electrons

Question 57

lattice energy

Answer 57

formation of ionic compounds gives off energy bc pe decreases with the formation of crystalline lattice of cations and anions

Question 58

ionic formulas

Answer 58

charges must balance

Question 59

naming ionic compounds

Answer 59

name of cation + base name of anion and -ide; if cation can form multiple charge add that

Question 60

metals that form cations with different charges

Answer 60

chromium, iron, cobalt, copper, tin, mercury, lead

Question 61

acetate

Answer 61

C2H3O2(-)

Question 62

carbonate

Answer 62

CO3(2-)

Question 63

hydrogen carbonate

Answer 63

HCO3(-)

Question 64

hydroxide

Answer 64

OH(-)

Question 65

Nitrite

Answer 65

NO2(-)

Question 66

Nitrate

Answer 66

NO3(-)

Question 67

Chromate

Answer 67

CrO4(2-)

Question 68

Dichromate

Answer 68

Cr2O7(2-)

Question 69

phosphate

Answer 69

PO4(3-)

Question 70

Hydrogen phosphate

Answer 70

HPO4(2-)

Question 71

dihydrogen phosphate

Answer 71

H2PO4(-)

Question 72

ammonium

Answer 72

NH4(+)

Question 73

hypochlorite

Answer 73

ClO(-)

Question 74

chlorite

Answer 74

ClO2(-)

Question 75

chlorate

Answer 75

ClO3(-)

Question 76

perchlorate

Answer 76

ClO4(-)

Question 77

permanganate

Answer 77

MnO4(-)

Question 78

Sulfite

Answer 78

SO3(2-)

Question 79

hydrogen sulfite

Answer 79

HSO3(-)

Question 80

sulfate

Answer 80

SO4(2-)

Question 81

hydrogen sulfate

Answer 81

HSO4(-)

Question 82

cyanide

Answer 82

CN(-)

Question 83

peroxide

Answer 83

O2(2-)

Question 84

hemi

Answer 84

0.50

Question 85

mono

Answer 85

1

Question 86

di

Answer 86

2

Question 87

tri

Answer 87

3

Question 88

tera

Answer 88

4

Question 89

penta

Answer 89

5

Question 90

hexa

Answer 90

6

Question 91

hepta

Answer 91

7

Question 92

octa

Answer 92

8

Question 93

nona

Answer 93

9

Question 94

deca

Answer 94

10