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College Chemistry I (CHMY 141) > Chem 1: Ch 5-9 UMT Dwyer > Flashcards

Chem 1: Ch 5-9 UMT Dwyer Flashcards

Midterm I

1
Q

Petrochemical

A

substance that is made from petroleum or other related substances such as coal or natural gas

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2
Q

Petroleum

A

a thick, flammable, yellow to black substance found in selected locations on earth, usualy in underground resevoirs; central to modern life in industrialized nations

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3
Q

water

A

clear, colorless, tasteless substance found almost everywhere on earth; essential to life support

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4
Q

petrochemical era

A

the period of time in which petrochemicals are used to manufacture products that are central to all aspects of life. generally agreed to have started inthe 1940s and is accelerating and continuing today

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5
Q

3 phases of matter

A

s, l, g

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6
Q

solid

A

constant shape and volume; vibration in a fixed position

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7
Q

liquid

A

variable shape (bottom of a container) and constant volume; touch one another & move around each other

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8
Q

gas

A

variable shape and volume (same as closed container); move independently, very widely spread

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9
Q

pure substance

A

one kind of matter, distinct and unue physical and chemical properties

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10
Q

mixture

A

sample of matter composed of 2 or more chemicals/substances; properties depend on relative amounts of parts
eg gin/water

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11
Q

element

A

a pure substance that cannot be decomposed into other pure substances by ordinary chemical means

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12
Q

compound

A

a pure substance that can be broken down into 2 or more pure substances by a chemical change.

Do NOT confuse element/compound with pure/mixture eg water is a pure compound that can be chemically separated into pure elemnts

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13
Q

physical properties

A

measurable and detecable by senses; eg water boils at 100*C

freezing point, boiling pt, density, color

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14
Q

physical change

A

new form of same substance

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15
Q

chemical properties

A

list of chemical changes possible; eg water reacts with sodium to form hydrogen, sodium ions, and hydroxide iions

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16
Q

chemcial change

A

old substance destroyed, new substance formed (eg hindenburg disaster)

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17
Q

homogenous

A

uniform appearance and composition throughout

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18
Q

heterogeneous

A

visibly different phases and/or different composition in a sample of matter

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19
Q

distillation

A

process of separating the components of a mixture by heating the liquid and collecting the gaseous components that sepearate formt he remainder of the liquid

separation of mix based on differences in volatility, speed of evaporation

element with lower boiling point evaporates first

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20
Q

3 major substances extracted from earth

A

petroleum, coal, natural gas

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21
Q

Pure substances that are compounds

A

water, sugar, baking soda, aspirin

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22
Q

pure elemental substances

A

gold, copper wire, lead fishing sinks

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23
Q

fractional distillation

A

The vapor enters the bottom fo the column and rises through the column, with the substances with the higher boiling points condensing back to the liquid state nearer the bottom of the columna and the lower-boiling liquids condensing higher in the column

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24
Q

cracking

A

less valuable fractions are subjected to a process called cracking- where the fraction is transformed, or cracked into gasoline

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25
Q

Macroscopic appearance… bubbles

A

the terms homogeneous and heterogeneous refer to the macroscopic appearance of a sample. a container fileld with ice and liquid water is hetergeneous in appearance but is also pure, as long as in both phases the water is pure

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26
Q

electrical charge

A

a property of matter that causes it to experienc a force when near other electrically chaged matter

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27
Q

2 types of charged matter

A
  1. attracted to the other type

2. same type repels the same type

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28
Q

Ben Franklin

A

proposed the hypothesis that the two types of charged matter resulted from an excess or deficiency of a single kind fo charge

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29
Q

Alessandro Volta

A

Italian Scientist- invented the first battery “voltaic pile” after learning that he itneraciton of brass and steel and a solution could cause a muscular contraction in a frog’s leg

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30
Q

Nicholson & Carlisle

A

used the current generated by a voltaic pile to decompose liquid water into hydrogetn and oxygen, finding that the volume of hydrogen produced was twice that of oxygen

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31
Q

Nicholson & Carlisle’s discovery led to…

A

Law of Combining Volumes

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32
Q

Law of Combining Volumes

A

the volume ratios in which gases react are always a ratio of small, whole numbers

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33
Q

Avogadro’s Hypothesis

A

explains the Law of Combining Volumes by proposing that equal volumes of gases contain equal numbers of molecules

led to distinguishing btwn monoatomic and diatomic elements based on the nature of the combining volumes

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34
Q

Monoatomic

A

Adjective
Consisting of one atom.
Monovalent.

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35
Q

Diatomic

A

Adjective

Consisting of two atoms.

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36
Q

“plum pudding” model

A

By 1911 the components of the atom had been discovered. The atom consisted of subatomic particles called protons and electrons. However, it was not clear how these protons and electrons were arranged within the atom. J.J. Thomson suggested the”plum pudding” model. In this model the electrons and protons are uniformly mixed throughout the atom:

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37
Q

Rutherford “gold foil” experiment

A

Rutherford tested Thomson’s hypothesis by devising his “gold foil” experiment. Rutherford reasoned that if Thomson’s model was correct then the mass of the atom was spread out throughout the atom. Then, if he shot high velocity alpha particles (helium nuclei) at an atom then there would be very little to deflect the alpha particles. He decided to test this with a thin film of gold atoms. As expected, most alpha particles went right through the gold foil but to his amazement a few alpha particles rebounded almost directly backwards.

These deflections were not consistent with Thomson’s model. Rutherford was forced to discard the Plum Pudding model and reasoned that the only way the alpha particles could be deflected backwards was if most of the mass in an atom was concentrated in a nucleus. He thus developed the planetary model of the atom which put all the protons in the nucleus and the electrons orbited around the nucleus like planets around the sun.

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38
Q

Rutherford “gold foil” experiment

A
  • discovered the proton via further experiments with alpha particles
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39
Q

What are the products when Nitrogen is bombarded with alpha particles?

A

protons are one product of the reaction

Oxygen

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40
Q

Who discovered the neutron?

A

many contributed, but it was Chadwick who ultimately conducted the highest quality experiments and interpreted the results correctly

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41
Q

What are the products when Berryllium is bombarded with alpha particles?

A

A particle with no charge and a mass similar to a proton

carbo

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42
Q

Electron

A 
e or e-
negative charge
mass= 9.109 x 10%-28g
0.000549 u     ~0
discovered in 1897 by Thomson
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43
Q

Proton

A 
p or p+
positive charge
mass= 1.673 x 10^-24
1.00728 u       ~1
discovered in 1919 by Rutherford
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44
Q

Neutron

A 
n or n0
zero charge
mass= 1.675 x 10^-24
1.00867 u      ~1
discovered in 1932 by Chadwick
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45
Q

Curvature of track is directly proportional to

A

the charge divided by (mass x velocity)

eg cloud chamber

46
Q

Cloud Chamber

A
  • charged particles leave a track
47
Q

compare the mass of a proton and an electron

A

if the mass of a proton =1 then comparatively, the mass of an electron is 1/2000

48
Q

What modern modifications have been made to Dalton’s Atomic Theory?

A
  1. atoms are made up of even smaller subatomic particles

2. atoms of an element can vary in mass

49
Q

Isotope

A

atoms of the same element with different #s of neutrons and thus different masses

eg H can have 0, 1 or 2 protons

50
Q

Nuclear symbol- what are the top and bottom numbers to the left of the chemical symbol?

A

the top left is the mass number, the bottom left is the atomic number

eg an Argon with 40 as the mass # is called Argon-40

51
Q

mass number

A

protons + # neutrons

52
Q

atomic #

A

of protons

53
Q

1 atomic mass unit (u) is defined as

A

1/12 the mass of a carbon-12 atom

also know as…
amu
u
Dalton

54
Q

6.02 x 10^23 u = ? g

A

1g

55
Q

Atomic mass

A

the average mass of the naturally occurring isotopes of an element, accounting for the relative abundance of each isotope

56
Q

Periodic Table

A

arrangement of elements according to atomic number left to right with elements with similar reactivities in columns. Each box in the periodic table has 3 items. The top most number isthe atomic #, the # of protons in atoms of that element. The centered symbol is the chemical symbolused to represent the element. The bottom # is the atomic mass of the naturally occurring isotopes of the element.

57
Q

Period

A

horizontal rows, numbered 1 (top) to 7 (bottom). usually not printed

58
Q

Group

A

vertical columns of elements with similar reactivity

U.S. numbering for Groups: “tall” columns are labeled A, and “ditch” columns are labeled B. The A groups are numbered 1-8 from left to right. The B groups are numbered 3-4-5-6-7-8-8-8-1-2

59
Q

Main group elements

A

U.S. A groups

60
Q

Transition elements

A

U.S. B groups

61
Q

stair step line

A

separates the metals on the left from the nonmentals on the right

62
Q

Modern defn of chemistry

A

the study of particles as large as molecules and as small as the subatomic particles proton, neutron, and electron

63
Q

Modern defn of biochemistry

A

the science that starts at the small end with molecules of biological relevance and continues up in size to the level of cells

64
Q

Chemical Nomenclature

A

the system by which substances are named

65
Q

IUPAC

A

The International Union of Pure and Applied Chemistry, the committee that recommends official names for all substances

66
Q

Elements that occur as diatomic in nature

A

H2, N2, O2, F2, Cl2, Br2, I2

Horses Need Oats For Cl ear Br own Iz

67
Q

Polyatomic molecules

A

(many atom)
Phosphorus P4
Sulfur S8

68
Q

Physical states of elements at 25*C and 1 bar…

A

Most are solids
11 gases: All 6 elements in Group 8A, H2, N2, O2, F2, Cl2
2 liquids: Hg, Br2

69
Q

Binary Molecular Compound

A

Compound formed by 2 nonmetals or a nonmetal and a metalloid (element that borders on the stair step line)

70
Q

How do you name binary molecular compounds?

A

A. First word is the name of the first element with a prefix to indicate the # of atoms of that element in the molecule

B. Second word is the name of the second element, changed to end in -ide, also with the appropriate prefix

71
Q

Prefixes & the number of atoms they indicate

A

mono = 1 di = 2 tri = 3 tetra = 4 penta = 5 hexa = 6 hepta = 7 octa = 8 nona = 9 deca = 10 if the compound is binary, then it ends in -ide

72
Q

How do u identify an isotope?

A

By its mass number, A, the total # of protons and neutrons in the nucleus

A = Z + N

73
Q

Interpolation

A

Predicting something within the range of your data

74
Q

Extrapolation

A

Predicting something beyond the range of your data

75
Q

Why r some atomic masses of elements inthe periodic table in parantheses?

A

They are radioactive, and there is no atomic mass in the sense that we have defined it. Instead, parantheses enclose the mass # of the most stable isotope

76
Q

1 u = ?g

A

1.66 x 10 ^-24 g

77
Q

7 diatomic elements

A

H2 N2 O2 F2 Cl2 Br2 I2

78
Q

Polyatomic molecules

A

Phosphorus P4

Sulfur S8

79
Q

Physical states of elements at 25*C

A

Most are solids
11 gases (group 8A) H2 N2 O2 F2 Cl2
2 liquids Hg Br2

80
Q

Noble gases

A 
Group 8A
He (g)
Ne (g)
Ar (g)
Kr (g)
Xe (g)
Rn (g)
81
Q

Binary molecular compound

A

Formed by 2 no metals or a nonmetal and…

82
Q

Metalloids

A

Border stair line

83
Q

How do you name a binary molecular compound?

A
  1. First word…
84
Q

Exceptions to binary molecular compound nomenclature rules

A

H2O is water… Not dihydrogen oxide

NH3 is ammonia …not nitrogen trihydride

85
Q

Which 2 diatomic elements have different state symbols?

A

Br2 (l)

I2 (s)

86
Q

Ion

A

Charged particle formed when a neutral atom or molecule loses or gains electrons

87
Q

Cation

A

Pos

Loses or gains e-

88
Q

Anion

A

Neg

When gains 1 or more electrons

89
Q

Monoatomic ion

A

Ion formed from a single atom

90
Q

Formula of a monatomic ion

A

Z

91
Q

Name of a monatomic ion

A

Name of element followed by the word ion

92
Q

Name of monatomic anion

A

-ide followed by the word ion

93
Q

Memorize common ions

A

Especially the group B with more than one
& Exceptions:
Zn2+
Ag+

94
Q

Naming acids

A
  • ic -> -ate

- ous -> -ite

95
Q

polyprotic acids

A

acids with more than one hydrogen ion

96
Q

Oxoacids Nomenclature: Prefix/Suffix

A 
per- -ic         one more O
-ic                the -ic acid
-ous             one fewer O
hypo- -ous    2 fewer O
hydro- -ic      NO O
97
Q

naming intermediate ions of a polyprotic acid: eg H3PO4

A

H3PO4 phosphoric acid
H2PO4 - dihyrdogen phosphate ion
HPO4 2- hydrogen phosphate ion
PO4 3- phosphate ion

98
Q

Ammonia v. Ammonium

A

NH3

steals H from somewhere & gets NH4+

99
Q

in pure water and in solutions, can one water molec react with another?

A

yes and it forms ions
H20 + H20 -> H3O+ + OH-
hydroxide ion
this only occurs to a very, very slight extent

100
Q

how do you name an ionic compound?

A

cation first then anion

101
Q

hydrate

A

ionic compound that contains water molecules

102
Q

Nomenclature: Element

Name; Formula

A

Name of element

Symbol of element; exceptions: H2, N2, O2, F2, Cl2, Br2, I2

103
Q

Nomenclature: Compounds made up of 2 nonmetals

Name; Formula

A
  • First element in a formula followed by second, changed to end in -ide, each element preceded by prefix to show the number of atoms in the molecule
  • Symbol of 1st element in name followed by symbol of second element, with subscript to show number of atoms in molecule
104
Q

Nomenclature: acid

Name; Formula

A

Most common: middle element changed to end in -UC
One more oxygen than -ic acid:add prefix per- to name of -ic acid
One fewer oxygen than ic acid: change ending of -ic acid to -ous
2 fewer oxygens than -ic acid: add prefix hypo- to name of -ous acid
No oxygen: prefix hydro- followed by name of 2nd element changed to end in -ic

H followed by symbol of nonmetal followed by O (if necessary), each with appropriate subscript.

Memorize:
Chloric acid: HClO3
Nitric acid: HNO3
Sulfuric acid: H2SO4
Carbonic acid: H2CO3
Phosphoric acid: H3PO4
105
Q

Nomenclature: monatomic cation

Name; Formula

A

Name of element followed by ion; if element forms more than one monatomic cation, elemental name is followed by ion charge in Roman numerals and in parentheses

Symbol of element followed by superscript to indicate charge

106
Q

Nomenclature: monatomic anion

Name; Formula

A

Name of element changed to end in -ide

Symbol of element followed by superscript to indicate charge

107
Q

Nomenclature: polyatomic anion from total ionization of oxoacid
Name; Formula

A

Replace -ic in acid name with -ate, or replace -ous in acid name with -ite, followed by ion

Acid formula without hydrogen plus superscript showing negative charge equal to number of hydrogens removed from acid formula

108
Q

Nomenclature: polyatomic anion from step-by-step ionization of oxoacid
Name; Formula

A

.

109
Q

Nomenclature: other polyatomic ions

Name; Formula

A

.

110
Q

Nomenclature: ionic compound

Name; Formula

A

.

111
Q

Ch9: A3

Explain how an anion can behave like an acid. Is it possible for a cation to be an acid?

A

An anion or cation that contains an ionizable hydrogen, such as HSO4- and NH4+ can lose the hydrogen as thus behave like an acid.

111
Q

Nomenclature: hydrate

Name; Formula

A

.

College Chemistry I (CHMY 141) (2 decks)

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