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Language, Culture, and Communication > Chem Exam 2 > Flashcards

Chem Exam 2 Flashcards

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1
Q

How to calculate the mass of a atom?

A

Protons and neutrons

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2
Q

What determines the energy of a nucleus?

A

electrons

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3
Q

Electromagnetic radiation is…

A

emitted energy

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4
Q

particles of electromagnetic radiation are…

A

photons

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5
Q

electron energy levels are…

A

lines in an atomic spectrum that are associated with the changes in energies of the electrons

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6
Q

when does the electron energy levels increase

A

when the neutrons and electrons are further from the nucleus

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7
Q

the number of sub levels in an energy level is equal to…

A

the principal quantum number of that energy level

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8
Q

orbital sublevels are

A

S (1 orbital), P (3 orbitals), D (5 orbitials)

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9
Q

How many electrons are in the s sublevel

A

2

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10
Q

How many electrons are in the p sub level

A

6

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11
Q

How many electrons are in the d sub level

A

10

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12
Q

ground state electron configurations are sued to…

A

indicate the placement of electrons in an atom and to find on periodic table

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13
Q

carbon electron configuration

A

1s^2 2s^2 2p^2

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14
Q

orbital boxes are…

A

the boxes used to show how electrons are arranged in the orbitals of an atom

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15
Q

The group number on the periodic tell the number of…

A

valence electrons for the elements

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16
Q

The lewis symbol represents…

A

the number of valence electrons as dots

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17
Q

atomic radius

A

distance between the nucleus and the outermost electrons

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18
Q

atomic size is determined by the atoms…

A

atomic radius

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19
Q

periodic table trends with the atomic radius

A

-increases from top to bottom
-decreases from left to right
-smallest in top right corner
-largest in bottom left corner

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20
Q

ionization energy

A

the energy required to remove one of the outermost electrons

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21
Q

cation

A

positive charged ion

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22
Q

anion

A

negative charged ion

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23
Q

ionization energy for metals

A

low

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24
Q

ionization energy for nonmetals

A

high

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25
Q

ionization energy on the periodic table

A

-decreases as you go down
-increases as you go to the right

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26
Q

metallic character

A

-what is more like a metal likes to give up electrons
-move prevalent in metals
-increases going down a group

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27
Q

chemical bonds

A

forms when atoms lose, gain, or share valence electrons to acquire a octet

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28
Q

ionic bonds

A

metal give to nonmetal

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29
Q

covalent bonds

A

nonmetal share with a nonmetal

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30
Q

positive ions

A

-metals lose electrons
-low ionization energy

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31
Q

negative ions

A

-nonmetals gain electrons
-high ionization energies

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32
Q

naming a cation

A

element + cation

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33
Q

naming a anion

A

element - change of ending + ide
oxygen-> oxide

34
Q

ionic compounds

A

consist of positive and negative charges held together by the strong electrical attractions between oppositely charged ions

35
Q

properties of ionic compounds

A

-solids at room temp
-high melting points

36
Q

formulas of ionic compounds the sum of ion charges equal to…

A

zero

37
Q

writing formulas of ionic compounds

A

the top charge goes to the bottom of the other element and vice versa

38
Q

naming ionic compounds

A

the metal is written 1st and has the same name and the nonmetal is second and has an ide ending

39
Q

ionic compound name for Mg3N2

A

magnesium nitride

40
Q

naming an ionic compound with metals with variable charge

A

a roman numeral equal to the ion charge is placed in () after metal name

41
Q

naming an ionic compound with metals with variable charge– Cu2+

A

Copper (II)

42
Q

polyatomic ions

A

a group of atoms with an overall charge

43
Q

properties of a polyatomic ion

A

-usually has a 1-,2-,3- charge
-often has a NM like phosphorus, sulfur, carbon, nitrogen, or oxygen

44
Q

OH-

A

hydroxide

45
Q

NH4+

A

ammonium

46
Q

NO3-

A

nitrate

47
Q

NO2-

A

nitrite

48
Q

ClO4-

A

perchlorate

49
Q

ClO3-

A

chlorate

50
Q

ClO2-

A

chorine

51
Q

ClO-

A

hypochlorite

52
Q

CO3^2-

A

carbonate

53
Q

HCO3-

A

hydrogen carbonate

54
Q

CN-

A

cyanide

55
Q

C2H3O2-

A

acetate

56
Q

SO4^2-

A

sulfate

57
Q

HSO4-

A

hydrogen sulfate

58
Q

SO3^2-

A

sulfite

59
Q

HSO3-

A

hydrogen sulfite

60
Q

PO4^3-

A

phosphate

61
Q

HPO4^2-

A

hydrogen phosphate

62
Q

H2PO4-

A

dihodrogen phosphate

63
Q

PO3^3-

A

phosphite

64
Q

prefixes for molecule compound 1

A

mono

65
Q

prefixes for molecule compound 2

A

di

66
Q

prefixes for molecule compound 3

A

tri

67
Q

prefixes for molecule compound 4

A

tetra

68
Q

prefixes for molecule compound 5

A

penta

69
Q

prefixes for molecule compound 6

A

hexa

70
Q

prefixes for molecule compound 7

A

hepta

71
Q

prefixes for molecule compound 8

A

octa

72
Q

prefixes for molecule compound 9

A

nona

73
Q

prefixes for molecule compound 10

A

deca

74
Q

Electronegativity non polar

A

0-0.4

75
Q

Electronegativity polar

A

.5-1.8

76
Q

Electronegativity ionic

A

1.8+

77
Q

Linear

A

2 bonded atoms

78
Q

trigonal planar trigonal planar

A

3 bonded atoms

79
Q

trigonal planar bent

A

2 bonded
1 lone pair

80
Q

tetrahedral tetrahedral

A

4 bonded pairs

81
Q

tetrahedral trigonal pyramidal

A

3 bonded pairs
1 lone pair

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