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CHE 103 > Final > Flashcards

Final Flashcards

1
Q

What best describes how an immunoassay interacts in a blood serum

A

It recognizes the 3D shape of a specific molecule

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2
Q

When electrons are shared between two atoms outer electron shells, what kind of bond forms

A

a covalent bond

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3
Q

How does the formation of a covalent bond occur?

A

by the overlap of two atoms electron orbitals

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4
Q

When a compound forms because an electron or electron is transferred from one element to another, it is referred to as what type of compound?

A

ionic

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5
Q

Briefly describe the term valance electron

A

a single electron (or one electron out of a pair) in the outer shell of an atom that is responsible for the chemical properties of the atom

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6
Q

how does the Lewis Theory explain the loss or gain of electrons in an ionic bond?

A

atoms are attempting to achieve a stable noble gas or “octet” electron configuration

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7
Q

What do the valance shells of all the noble gas elements have in common

A

all have 8 electrons

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8
Q

As you move from the top to the bottom of the periodic table, what happens to the electronegativity of the elements

A

it decreases

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9
Q

How is the Br-H bond categorized?

A

polar covalent bond

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10
Q

Non polar covalent bonds

A

-occurs when the electronegativity of both atoms is equal

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11
Q

polar covalent bonds

A

-occurs when the difference in electronegativity is between .4 and 1.9

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12
Q

What is the electronegativity difference between the C-O bond? (C- 2.5, O- 3.5)

A

1.0

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13
Q

Many organic compounds have numerous C-H bonds. What is the average difference in electronegativity in one of them? (C- 2.5 ,H- 2.1)

A

0.4

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14
Q

How many bonds does carbon normally form?

A

4

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15
Q

How is ethane best represented by a lewis structure?

A

2 carbons that are bonded (C-C) with 3 bonds attached to each carbon

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16
Q

What is the formula for an alkane with ten carbons, decane

A

C10H22

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17
Q

Propane C3H8 is best represented by which lewis structure?

A

2 zig zag lines

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18
Q

Draw lweis structure for ethene C2H2 (a.k.a ethylene). How many double bonds does it have?

A

1

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19
Q

How many bonds does each carbon atom in an alkene normally have?

A

2 (double-bonded carbon and 2 single bonded elements)

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20
Q

meth-

A

1 carbon

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21
Q

eth-

A

2 carbons

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22
Q

prop-

A

3 carbons

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23
Q

but-

A

4 carbons

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24
Q

pent-

A

5 carbons

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25
Q

hex-

A

6 carbons

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26
Q

hept-

A

7 carbons

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27
Q

oct-

A

8 carbons

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28
Q

non-

A

9 carbons

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29
Q

dec-

A

10 carbons

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30
Q

alkanes

A

single bond

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31
Q

alkenes

A

double bonded carbon

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32
Q

alkynes

A

triple bonded carbon

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33
Q

How many carbon atoms should be in the molecule pentyne

A

5

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34
Q

How many carbon atoms should be in the molecule octanol

A

8

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35
Q

Ketone

A

R-(O=C)-R

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36
Q

Ketone end in

A

-one

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37
Q

alkanes end in

A

-ane

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38
Q

alkenes end in

A

-ene

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39
Q

alkynes end in

A

-yne

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40
Q

cycloalkanes

A

make rings (all elements are bonded to each other like a circle) (each point is a carbon)

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41
Q

cycloalkanes begin with

A

cyclo (wit prefix (meth, but, eth) before the cyclo)

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42
Q

ether

A

R-O-R

43
Q

ether compounds end in

A

oxy

44
Q

Esters

A

R-O-(C=O)-R

45
Q

esters end in

A

-yl

46
Q

alcohol

A

R-OH

47
Q

alcohols end in

A

-ol

48
Q

aldehyde

A

R-(C=O)-H

49
Q

aldehydes end in

A

-al

50
Q

carboxylic acid

A

R-(C=O)-OH

51
Q

carboxylic acid end in

A

-oic acid

52
Q

A double bonded alcohol compound with 4 carbons is called

A

methenol

53
Q

COCl2 is an example of what type of electron-domain

A

tetrahedral

54
Q

PF3 is an example of what type of electron-domian

A

trigonal pyramidal (<109.5)

55
Q

a tetrahedral is bent at what angle

A

109.5

56
Q

linear angle

A

180

57
Q

Trigonal planar angle

A

120

58
Q

SO3 is an example of what type of electron-domian

A

Trigonal planar

59
Q

Solid

A

definite shape and definite volume, not compressible

60
Q

Liquids

A

have no definite shape but do have a definite volume, able to flow

61
Q

Gases

A

have no definite shape or volume. molecules very far apart (highly compressible)

62
Q

Mixture

A

blending two or more “pure substances with variable composition

63
Q

Pure substance

A

the components cannot be separated by any physical means (distilation etc.)

64
Q

Elements

A

the simplest type of substance with unique physical and chemical properties. Consists of only one type of atom and cannot be broken down into simpler substances by any means (physical or chemical)

65
Q

Compounds

A

structures that consist of two or more atoms that are chemically bound together and thus behave as an independent unit (ex. CO2)

66
Q

Homogeneous Mixture

A

has the same properties and composition throughout the sample (ie. Salt water or brine is an aqueous homogeneous)

67
Q

Heterogeneous Mixture

A

consists of two or more phases of variable composition that differ in properties (ie. water floating in oil)

68
Q

Who created the periodic table

A

Dmitri Mendeleev

69
Q

What are the three element classification

A

Metals, Nonmetals and metalloids

70
Q

Metals Physical properties

A
  • conduct heat/electricity
    -solid (often hard except Hg)
    -Metallic luster or shine
    -Malleability (sheets) and ductility (wires)
71
Q

Metals chemical properties

A

-released electrons to form cations

72
Q

Nonmetals physical properties

A

-often gases (Br is a liquid)
- do not conduct
-brittle solids, dull appearance
- S, I, C, P (solids)

73
Q

Nonmetals Chemical properties

A

-react with metals
-gain electron to form anions

74
Q

Metalloids physical properties

A

-solids
-semiconductors
- ie. Si can conduct electricity at hight temps

75
Q

Metalloids chemical properties

A

-form a variety of ionic, electron-deficient compounds

76
Q

Which of the following states of matter is generally considered the most ordered?

A

solids

77
Q

Cu

A

Copper

78
Q

Ag

A

Silver

79
Q

Au

A

Gold

80
Q

Fe

A

Iron

81
Q

chemical properties

A

substance’s potential to react with some other substances in its environment (ie. flammability, corrosiveness etc.)

82
Q

Physical properties

A

properties measured without changing the chemical composition of the substance (ie. boiling point, freezing point)

83
Q

Chemical changes

A

matter undergoes chemical changes to produce new substances

84
Q

Types of chemical changes

A

-iron rusting
-burning wood
-metabolism
-cooking an egg
-baking a cake
-electroplating
-rotting banana
-vinegar and baking soda solution
-fireworks
-chemical battery

85
Q

physical changes

A

changes of a substance between different forms of matter

86
Q

Physical changes examples

A

-crushing a can
-melting an ice cube
-boiling water
-mixing sand and water
-breaking glass
-dissolving sugar in water
-shredding paper
-chopping wood
-mixing green and red marbles
-sublimation of dry ice

87
Q

denisty =

A

mass / volume

88
Q

density

A

ratio of an objects mass to its volume

89
Q

atomic theory

A

-all matter is made up of tiny, invisible particles called atoms
-atoms cannot be created, destroyed, or transformed into other atoms in a chemical reaction
-all atoms of a given element are identical
-atoms combine in simple, whole-number ratios to form compounds

90
Q

the law of multiple proportions

A

any time two or more elements combine in different ration, different compounds are formed

91
Q

what is Ernest rutherford known for

A

the gold foil experiment

92
Q

what are the three subatomic particles

A

electrons, neurons and protons

93
Q

what are the 4 orbitals

A

s, p, d, f

94
Q

Which orbital has the most energy

A

f

95
Q

Which orbital has the least energy

A

s

96
Q

s orbitals are (blank) shaped

A

spherically

97
Q

p orbitals are (blank) shaped

A

dumbell

98
Q

Group 1 (column 1) is what group

A

alkali metals

99
Q

Group 2 (column 2) is what group

A

alkaline earth metals

100
Q

group 17 (column 17) is what group

A

halogens

101
Q

group 18 (column 18) is what group

A

noble gas

102
Q

covalent bond

A

2 non metals

103
Q

ionic bonds

A

have 1 metal and 1 nonmetal

104
Q

valance bond theory

A

predicts that two nonmetals atoms will share electron in a covalent bond when there atomic orbitals overlap

CHE 103 (3 decks)

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