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Chemistry 121 > Exam 2 blocks 4-6 > Flashcards

Exam 2 blocks 4-6 Flashcards

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1
Q

What is the periodic table?

A

a graphical representation of all the known elements

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2
Q

What does periodic law state?

A

when elements are arranged according to increasing atomic number, elements having similar properties fall into place at regularly occurring intervals on the P table

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3
Q

Where are you most likely to find an element with similar properties?

A

the same vertical column

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4
Q

What are the periods on the periodic table?

A

the horizontal rows on the table numbered 1-7

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5
Q

What element numbers are the lanthanides?

A

58-71

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6
Q

What element numbers are the actinides?

A

90-103

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7
Q

What are lanthanides and actinides collectively called?

A

inter transition elements

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8
Q

What are the vertical columns on the periodic table?

A

groups labled IA-VIIIA

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9
Q

All but what group are known as representitive elements?

A

VIIIA

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10
Q

All elements accept H in group IA are called?

A

Alkali metals

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11
Q

What is the name of group IIA?

A

Alkaline Earth Metals

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12
Q

What are the elements in group VIIA?

A

Halogens

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13
Q

What are the elements in group VIIIA?

A

Noble Gasses.

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14
Q

What is group B referred to?

A

transition elements

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15
Q

How many metaloids are there?

A

8

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16
Q

What are noble elements?

A

Elements that are unreactive and usually found in an uncombined state

Au,Ag, Pd, Pt, Ta

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17
Q

What are the most unreactive of all of the elements?

A

The noble gasses

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18
Q

How many elements are solid at room temp?

A

104

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19
Q

What are the two types of solids?

A

Crystalline

Amorphous

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20
Q

What is a crystalline solid?

A

solids that have Very predictable, repeating, densely packed structures

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21
Q

What two elements are liquid at room temp?

A

Bromine and Mercury

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22
Q

Which noble gas is the most dense?

A

Xe Xenon

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23
Q

How many elements are gasses at room temp?

A

11

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24
Q

Minimum energy equals ____?

A

maximum stability

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25
Q

Principal energy levels are also called?

A

Shells

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26
Q

What are the three divisions of shells

A

shells
subshells
orbitals

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27
Q

What is a shell?

A

A region of space containing electrons that spend most of their time approx. the same distance from the nucleus and have similar energies

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28
Q

What is the maximum number of electrons that any shell can hold?

A

2n^2

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29
Q

The maximum number of subshells within a shell is the same as?

A

the shell number

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30
Q

What are the four letters in order assigned to subshells?

A

S
P
D
F

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31
Q

How many electrons can a S shell hold at max?

A

2

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32
Q

How many electrons can a P shell hold at max?

A

6

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33
Q

How many electrons can a D shell hold at max?

A

10

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34
Q

How many electrons can a F shell hold at max?

A

14

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35
Q

How many electrons at max can be in an orbital?

A

2

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36
Q

How many orbitals does an S shell have?

A

1

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37
Q

How many orbitals does an P shell have?

A

3

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38
Q

How many orbitals does an D shell have?

A

5

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39
Q

How many orbitals does an F shell have?

A

7

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40
Q

What does it mean for an electron to be degenerate?

A

It has the same energy level as the other electrons within the same subshell

41
Q

What does the pauli exclusion principal state?

A

that electrons in the same orbital must have opposite spins

42
Q

What are the two parts of hunds rule?

A

1) All orbitals in the same subshell will get one electron before any electrons are paired in an orbital
2) Unpaired electrons in the same subshell will all have the same spin

43
Q

What are the two types of chemical compounds?

A

Ionic compounds

Molecular Compound

44
Q

What are ionic compounds composed of?

A

Formula units

45
Q

What are formula units composed of?

A

Ions

46
Q

What is another work for molecular compounds?

A

covalent

47
Q

What are molecular compounds composed of?

A

molecules

48
Q

What are molecules composed of?

A

charge neutral atoms

49
Q

What is a chemical bond?

A

The attractive force that chemically bonds atoms or ions into complex units

50
Q

What are the two types of chemical bonds?

A

Ionic and covalent

51
Q

What does ionic bonding require?

A

a transfer of electrons

52
Q

What happens to a charge if electrons are lost?

A

it becomes positive

53
Q

What happens to a charge if electrons are gained?

A

it becomes negative

54
Q

What is a cation?

A

a positively charged ion

55
Q

What is an anion?

A

a negatively charged ion

56
Q

WHat are the two conditions for an ionic bond?

A

the charges must be opposite and of the same magnitude

57
Q

Why do ions form?

A

The quest for an octet of valence electrons and greater stability

58
Q

What is electronegativity?

A

the numerical measure of the attractive force an atom has for electrons

59
Q

Define formula unit

A

The smallest whole-number repeating ratio of ions present in an ionic compound that results in charge nutrality

60
Q

Which is bigger, a cation or an anion? why

A

An anion is bigger because it gains electrons to become an anion. more electrons = higher volume

61
Q

Ions ___ elections

Molecules___electrons

A

Transfer

Share

62
Q

How many electrons to form one covalent bond?

A

2

1 pair

63
Q

What increases electron density?

A

When electrons are localized

64
Q

High electron density = ?

A

High strength

65
Q

What is a molecular orbital?

A

A unique orbit formed when tow atomic orbits come together

66
Q

What is hybridization?

A

The process in which two atomic orbits overlap and form a new molecular orbit

67
Q

What are two ways the strength of a covalent bond can be increased?

A

Decreasing the area in which the electrons are localized

placing more electrons into the same area forming multiple bonds

68
Q

How many electrons are involved per bond?

A

2

69
Q

What are lone pair electrons?

A

valence electrons not involved in a bond

70
Q

what are bonding electrons?

A

electrons involved in a bonding pair

71
Q

What bond shares electrons?

A

Covalent

72
Q

What bond transfers electrons?

A

ionic

73
Q

Which type of bond involves all valence electrons?

A

ionic

74
Q

Which type of bond forms between similar atoms?

A

covalent

75
Q

Which type of bond forms between dissimilar atoms?

A

ionic

76
Q

What compounds are formed from formula units?

A

Ionic

77
Q

What compounds are formed from molecules?

A

Covalent

78
Q

What bond can form multiple bonds?

A

covalent

79
Q

What bond can only for single bonds?

A

Ionic

80
Q

IN which bond do bonded electrons hybridize?

A

covalent

81
Q

In what instances are the electrons in a covalent molecular orbital shared equally?

A

Homoatomic Diatomic elements

82
Q

What causes the unequal sharing of electrons in covalent bonds?

A

slight variations in the electronegativity

83
Q

Which side of a polar covalent bond is negative

A

the side with the highest electronegativity

84
Q

Are polar molecules charged?

A

no. The negative and positive charges are both of equal intensity and cancel each other out

85
Q

Which bonds have a large difference in electronegativity?

A

ionic

86
Q

Which bonds have small differences in electronegativity?

A

polar covalent

87
Q

Which bonds have no difference in electronegativity?

A

non-polar covalent bonds

88
Q

If the difference in electronegativity is zero then the bond is?

A

non-polar covalent

89
Q

If the difference in electronegativity is between zero and 1.5, then the bond is?

A

polar covalent

90
Q

If the difference in electronegativity is greater than 2, the bond is

A

Ionic

91
Q

If the difference in electronegativity is between 1.5 and 2 and there is no metal in the bond then the bond is?

A

polar-covalent

92
Q

If the difference in electronegativity is between 1.5 and 2 and there is metal in the bond then the bond is?

A

Ionic

93
Q

As bond strength increases the bond take son more ___ characteristics

A

Ionic

94
Q

What causes Molecular polarity?

A

The presence of polar bonds and the way they are arranged in the molecule

95
Q

When is a molecule non-polar?

A

if the molecule has no polar bonds

or if the polar bonds in the molecule are arranged in a way that the polar charges cancel each other out

96
Q

What does the Pauli exclusion principle state?

A

Electrons in the same orbital must have opposite spins

97
Q

What are the two parts to Hunds rule?

A

1-all orbitals within the same su shell will get one electron before any electrons are paired in an orbital

2-unpaired electrons in the same subshell will have the same spin

98
Q

What does the octet rule state?

A

When forming ions, atoms lose or gain e- in such a way so that their e- configuration will match the noble gas closest to them in the periodic table

Chemistry 121 (6 decks)

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