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ALL 11th GRADE CLASSES > CHEMISTRY REGENTS REVIEW ALL TOPICS > Flashcards

CHEMISTRY REGENTS REVIEW ALL TOPICS Flashcards

1
Q

which statement describes the earliest model of the atom

1) an atom is an invisible hard sphere

2) an atom has a small dense nucleus

3) electrons are negative particles in an atom

4) electrons in an atom have wavelike properties

A

1

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2
Q

in all atoms of bismuth the number of electrons must equal the

number of protons

number of neutrons

sum of the number of neutrons and protons

difference between the number of neutrons and protons

A

1

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3
Q

an orbital is a region in an atom where there is a high probabitlity of finding

an alpha particle

an electron

a neutron

a positron

A

2

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4
Q

which electron shell in an atom of calcium in the ground state has an electron with the greatest amount of energy

1
2
3
4

A

4

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5
Q

as the elements in period 2 are considered in order from lithium to flourine, there is an increase in the

atomic radius

electronegativity

number of electron shells

number of electrons in the fist shell

A

2

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6
Q

which element is classified as a metalloid

boron

potassium

sulfur

xenon

A

boron

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7
Q

strontium and barium have similar chemical properties because atoms of these elements have the same number of

protons
neutrons
electron shells
valance electrons

A

valance electrons

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8
Q

which term represents the fixed proportion of elements in a compound

atomic mass
molar mass
chemical formula
density formula

A

chemical formula

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9
Q

which two terms represent types of chemical formulas

mechanical and structural

mechanical and thermal

molecular and structural

molecular and thermal

A

3

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10
Q

which element has metallic bonds at room temp

bromine

cesium

krypton

sulfur

A

cesium

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11
Q

what is the number of electrons shared between the atoms in a molecule of nitrogen, N2

8
2
3
6

A

6

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12
Q

given the equation representing a reaction
H + H yeilds H2
what occurs during this reaction?

a bond is broken and energy is absorbed

a bond is broken and energy is released

a bond is formed and energy is absorbed

a bond is formed and energy is released

A

4

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13
Q

an atom of which element has the strongest attraction for electrons in a chemical bond

chlorine
carbon
phosphorus
sulfur

A

chlorine

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14
Q

at STP, a 50 gram sample of H2O (l) and a 100 gram sample of H2O (l) have

the same chemical properties
the same volume
diff temperatures
diff empirical formulas

A

1

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15
Q

what statement describes a mixture of sand and water at room temperature

it is heterogeneous and its components are in the same phase

it is heterogeneous and its componets are in different phases

it is homogenous and its componets are in the same phase

it is homogenous and its components are in different phases

A

2

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16
Q

distillation is a process used to separate a mixture of liquids based on different

boiling points
densities
freezing points
solubilities

A

boiling points

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17
Q

according to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas

the particles are constantly moving in circular patterns

the particles collide decreasing the total energy in the system

the particles have attractive forces between them

the particles are considered to have negligible volume

A

4

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18
Q

for a chemical system at equilibrium the concentrations of both the reactants and the products must

decrease
increase
be constant
be equal

A

constant

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19
Q

in terms of disorder and energy, systems in nature have a tendency to undergo changes toward

less disorder and lower energy

less disorder and higher energy

greater disorder and lower energy

greater disorder and higher energy

A

3

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20
Q

the only two elements in alkenes and alkynes are

carbon and nitrogen

carbon and hydrogen

oxygen and nitrogen

oxygen and hydrogen

A

2

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21
Q

which functional group contains a nitrogen atom and an oxygen atom

ester
ether
amide
amine

A

amide

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22
Q

when a sample of Mg (s) reacts completely with O2(g), the Mg(s) loses 5 moles of electrons. How many moles of electrons are gained by the O2(g)

1 mol
2.5 mol
5 mol
10 mol

A

5 mol

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23
Q

which statement describes the reactions in an electrochemical cell

oxidation occurs at the anode and reduction occurs at the cathode

oxidation occurs at the cathode and reduction occurs at the anode

oxidation and reduction both occur at the cathode

oxidation and reduction both occur at the anode

A

1

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24
Q

what is the color of bromcresol green indicator in a solution with a pH value of 2

blue
green
red
yellow

A

4

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25
Q

in which reaction is an atom of one element converted into an atom of another element

combustion
fermentation
oxidation-reduction
transmutation

A

4

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26
Q

in which type of nuclear reaction do nuclei combine to form a nucleus with a greater mass

alpha decay
beta decay
fusion
fission

A

fusion

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27
Q

which electron configuration represents the electrons in an atom of sulfur in an excited state

2-8-6
2-7-7
2-8-7
2-7-8

A

2

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28
Q

which notations represent atoms that have the same number of protons but a different number of neutrons

H-3 and He-3
S-32 and S-32
Cl-35 and Cl-37
Ga-70 and Ge-73

A

3

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29
Q

what is the molarity of 2 liters of an aqueous solution that contains .5 mole of potassium iodide, KI

1 M
2 M
.25 M
.5 M

A

.25 M

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30
Q

hydrochloric acid reacts faster with powdered zinc than with an equal mass of zinc strips because the greater surfact are of the powdered zinc

decrease the frequency of particle collisions

decreases the activation energy of the reaction

increases the frequency of particle collisions

increases the activation energy of the reaction

A

3

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31
Q

which radioisotope requires long term storage as the method of disposal to protect living things from radiation exposure over time

Pu-239
Fr-220
Fe-53
P-32

A

1

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32
Q

state the number of protons in an atom of N-15

A

7

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33
Q

state the number of electrons in each shell of an N-14 atom in the ground state

A

2-5

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34
Q

based on the atomic mass of the element nitrogen on the periodic table compare the relative abundances of the naturally occuring isotopes of nitrogen

A

the relative abundances of the naturally occuring isotopes of N-14 is more abundant than N-15

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35
Q

which statement describes a concept included in the wave mechanical model of the atom

protons neutrons and electrons are located in the nucleus

electrons orbit the nucleus in shells at fixed distances

atoms are hard invisible spheres

electrons are located in regions called orbitals

A

4

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36
Q

as an electron in an atom moves from a higher energy state to a lower energy state, the atom

becomes a negative ion

becomes a poisive ion

releases energy

absorbes energy

A

3

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37
Q

two atoms that are different isotopes of the same element have

the same number of protons and the same number of neutrons

the same number of protons but a different number of neutrons

a different number of protons but the same number of neutrons

a different number of protons and a different number of neutrons

A

2

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38
Q

the element in group 14 period 3 of the periodic table is classified as a

metal
noble gas
metalloid
nonmetal

A

3

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39
Q

which conclusion was developed as a result of the gold foil experiment

atoms are mostly empty space

all atoms are hard invisible spheres

atoms have different volumes

all atoms have the same volume

A

1

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40
Q

which two particles each have a mass approximately equal to one atomic mass unit

positron and proton

positron and electron

neutron and electron

neutron and proton

A

4

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41
Q

an excited potassium atom emits a specific amount of energy when one of its electrona moves from

the first shell to the fourth shell

the second shell to the fourth shell

the fourth shell to the fifth shell

the fourth shell to the second shell

A

4

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42
Q

which list of elements includes a metal, a metalloid, and a noble gas?

Rd, Cl, Ne
Rn, Cl, Ne
Sr, Si, Rn
Si, Rb, Sr3

A

3

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43
Q

which element has the lowest density at 298K and 101.3kPa

argon
fluorine
nitrogen
oxygen

A

3

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44
Q

which statement describes the changes in bonding and energy that occur when a molecule of iodine forma two separate atoms of iodine

a bond is formed as energy is absorbed

a bond is formed as energy is released

a bond is broken as energy is absorbed

a bond is broken as energy is released

A

3

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45
Q

the degree of polarity in the bond between a hydrogen atom and an oxygen atom in a molecule of water can be assessed using the difference in

densities
electronegativities
melting points
intermolecular forces

A

2

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46
Q

which substance can not be broken down by a chemical change

ammonia
krypton
ethanol
water

A

2

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47
Q

which term is used to express the concentration of an aqueous solution

parts per million
heat of fustion
pressure at 0 degrees C
volume at 0 degrees C

A

1

48
Q

which process represents a chemical change

iodine sublimes
water evaporates
an ice cube melts
a candle burns in air

A

4

49
Q

systems in nature tend to undergo changes toward

higher energy and higher entropy
higher energy and lower entropy
lower energy and higher entropy
lower energy and lower entropy

A

3

50
Q

which statement describes the bonding in an alkyne molecule

there is at least one carbon to carbon double bond

there is at least one carbon to carbon triple bond

there is at least one carbon to oxygen single bond

there is at least one carbon to oxygen double bond

A

2

51
Q

which term identifies a type of organic reaction

deposition
distillation
polymerization
vaporization

A

3

52
Q

in an electrochemical cell, oxidation occurs at the

anode
cathode
salt bridge
switch

A

anode

53
Q

which energy conversion occurs in an operating electrolytic cell

chemical energy to electrical energy

electrical energy to chemical energy

nuclear energy to electrical energy

electrical energy to nuclear energy

A

2

54
Q

one acid base theory states that a base is an

H- donor
H- acceptor
H+ donor
H+ acceptor

A

4

55
Q

the acidity or alkalinity of a solution can be measured by its

pH value
electronegativity value
boiling point
freexing point

A

1

56
Q

which nuclear emission has the greatest mass

positron
gamma ray
beta particle
alpha particle

A

4

57
Q

which statement describes the net change that occurs during nuclear fission

electrons are converted to protons

protons are converted to electrons

mass is converted to energy

energy is converted to mass

A

3

58
Q

which general trend is observed as the elements in period 2 are considered from left to right

atomic mass decreases

melting point increases

electronegativity increases

first ionization energy decreases

A

3

59
Q

one mole of bromine gas, Br2, has a mass of

35 g
70 g
79.9 g
159.8 g

A

4

60
Q

which sattement describes the charge and the radius of the magnesium ion formed when a magnesium atom loses two electrons

the Mg ion is postive and has a radius larger than the Mg atom

the Mg ion is negative and has a radius larger than the Mg atom

the Mg ion is positive and has a radius smaller than the Mg atom

the Mg ion is negative and has a radius smaller than the Mg atom

A

3

61
Q

the concept that matter is composed of tiny, discrete particles is generally attributed to the

greeks
romans
english
germans

A

greeks

62
Q

the first subatomic particle discovered was the

proton
neutron
electron
photon

A

electron

63
Q

According to the law of the conservation of mass, if the products of a reaction have a mass of 64 g, then the total mass of the reactants

must be less than 64g

must be equal to 64g

must be more than 64g

is not related to the mass of the products

A

2

64
Q

the gold foil experiment led scientists to conclude that an atoms

positive charge is evenly distributed throughout its volume

negative charge is mainly concentrated in its nucleus

mass is evenly distributed throughout its volume

volume is mainly unoccupied

A

4

65
Q

the model of the atom that pictured the atom with electrons stuch randomly throughout the mass of the atom was called the

cannonball model

plum pudding model

planetary model

wave mechanical model

A

2

66
Q

after bombarding a gold foil sheet with alpha particles scientists concluded that atoms mainly consist of

electrons
empty space
protons
neutrons

A

empty space

67
Q

experimental evidence indicates that the nucleus of an atom

contains most of the mass of the atom

contains a small percentage of the mass of the atom

has no charge

has a negative charge

A

1

68
Q

daltons atomic theory states that

all atoms of an element are positively charged

different elements can have the same mass

atoms of a given element must be identical

all the atoms in a compound are identical

A

3

69
Q

modern theory pictures an electron as

a particle

a wave only

both a particle and a wave

neither a particle nor a wave

A

3

70
Q

why did rutherford conclude that the atom was mostly empty space

A

most alpha particles went through it

71
Q

the atomic mass of an element is defined as the weighted average mass of that elements

most abundant isotope

least abundant isotope

naturally occuring isotopes

radioactive isotopes

A

3

72
Q

element x has two isotopes. if 72% of the element has an isotopic mass of 84.9 amu and 28% has an isotopic mass of 87 amu, the average atomic mass of element X is numerically equal to

(72 + 98.9)(28 + 87)
(72 - 84.9)(28 - 87)
(.720)(84.9) + (.280)(87)
(72)(84.9) + (28)(87)

A

3

73
Q

a neutral atom with 6 electrons and 8 neutrons is an isotope of

carbon
silicon
nitrogen
oxygen

A

1

74
Q

the major portion of an atoms mass consists of what

A

neutrons and protons

75
Q

a neutron has approximately the same mass as

an alpha particle
a beta particle
an electron
a proton

A

4

76
Q

what is the nuclear cahrge of an atom with a mass of 23 and an atomic number of 11

11
12
23
34

A

11

77
Q

compared to the charge and mass of a proton, an electron has

the same charge and a smaller mass

the same charge and the same mass

an opposite charge and a smaller mass

an opposite charge and the same mass

A

3

78
Q

which of the following statements are correct

a proton is positively charged and a neutron is negatively charged

a proton is negatively charged and a neutron is positively charged

a proton is positively charged and an electron is negatively charged

a proton is negatively charged and an electron is positively charged

A

3

79
Q

when electrons in an excited state fall to lower energy levels, energy is

absorbed
released
neither absorbed nor released
both absorbed and released

A

2

80
Q

the characteristic bright line spectrum of an atom is produced when

nuclei undergo fission

nuclei undergo fusion

electrons move from higher to lower levels

electrons move from lower to higher energy levels

A

3

81
Q

when the electrons of an excited atom fall back to lower energy levels, the emission of energy produces

beta particles
alpha particles
spectral lines
gamma radiation

A

3

82
Q

which atom in the ground state contains one completely filled p orbital

Ne
O
He
Be

A

1

83
Q

hat is the total number of electrons in the second principal energy level of a calcium atom in the ground state

6
2
8
18

A

8

84
Q

the atom of which element in the ground state has two unpaired electrons in the 2p sublevel

Fl
N
Be
C

A

C

85
Q

what is the toal number of occupied s orbitals in an atom of nickel in ground state

1
2
3
4

A

4

86
Q

which atom in hte ground state has only three electrons in the 3p sublevel

phosphorus
potassium
argon
aluminum

A

1

87
Q

what is the total number of occupied principal energy levels in a neutral atom of neon in the ground state

1
2
3
4

A

2

88
Q

in an atom of lithium in the ground state, what is the total number of orbitals that contain only one electron

1
2
3
4

A

1

89
Q

which of the following cannot be decomposed by chemical means

sodium
ethanol
sucrose
water

A

sodium

90
Q

a compound differs from an element in that a compound is

homogenous

has difinite composition

has a definite melting point

can be decomposed by a chemical reaction

A

4

91
Q

a compound differs from a mixture in that a compound always has a

homogenous composition
maximum of two elements
minimum of three elements
heterogenous composition

A

1

92
Q

a pure substance that is composed only of identical atoms is classified as

a compound

en elements

a heterogeneous mixture

a homogenous mixture

A

2

93
Q

most elements are

metals
nonmetals
gases
made in a laboratory

A

1

94
Q

which is a characteristic of all mixtures

they are homogenous
they are heterogeneous
their compositions are in a definite ratio
their compositions may vary

A

4

95
Q

a heterogeneous material may be

an element
a compound
a pure substance
a mixture

A

4

96
Q

which of these materials is a mixture

water
air
methane
magnesium

A

2

97
Q

each particle contained in hydrogen gas is made up of two identical hydrogen atoms chemically joined together. Hydrogen gas is

a compound

an element

a homogenous mixture

a heterogeneous mixture

A

an elements

98
Q

which of the following materials is a pure substance

air
water
fire
earth

A

2

99
Q

which statement is an identifying characteristic of a mixture

a mixture can consist of a single element

a mixture can be separated by physical means

a mixture must have a definite composition by weight

a mixture must be homogenous

A

2

100
Q

which substance can be decomposed by a chemical change

ammonia
aluminum
magnesium
manganese

A

ammonia

101
Q

a model of the atom that pictured the atom with electrons traveling in circular orbit was called the

planetary model
cannonball model
wave mechanical model
plum pudding model

A

1

102
Q

compared to the entire atom, the nucleus of the atom is

smaller and contains most of the atoms mass

smaller and contains little of the atoms mass

large and contains most of the atoms mass

large and contains little of the atoms mass

A

1

103
Q

neutral atoms must contain equal number of

protons and electrons
protons and neutrons
protons, neutrons, and electrons
neutrons and electrons

A

1

104
Q

compared with an electron a proton has

more mass and the same charge

more mass and an opposite charge

equal mass and the same charge

equal mass and an opposite charge

A

2

105
Q

the total number of electrons in a neutral atom of any element is always equal to the atoms

mass number
number of neutrons
number of protons
number of nucleons

A

3

106
Q

all isotopes of neutral atoms of sodium have

11 protons and 12 neutrons

12 protons and 11 neutrons

11 protons and 11 electrons

12 protons and 12 electrons

A

3

107
Q

an atom in the excited state contains

more electrons than an atom in the ground state

more protons than an atom in the ground state

more potential energy than an atom in the ground state

more mass than an atom in the ground state

A

3

108
Q

which of the following particles has the smallest mass

neutron
electron
proton
hydrogen atom

A

2

109
Q

a chemical formula is an expression used to represent

mixtures only
elements only
compounds only
elements and compounds

A

4

110
Q

which formula represents a compound

Ca
Cr
CO
Co

A

3

111
Q

What is the total number of atoms in the formula Ca(NO3)2

7
2
3
9

A

9

112
Q

pure nitrogen combines directly with an active metal to form a

nitrate
nitride
nitrite
permanganate

A

2

113
Q

Ag + Hsub2S yeilds Agsub2S +H sub

what is the sum of the coefficients when teh equation is completely balanced using the smallest whole number coefficients

5
8
10
4

A

5

114
Q

pure oxygen reacts with metals to form

oxalates
oxalites
oxides
oxygenates

A

3

115
Q

which of the following is the formula of a compound

Fr
Mn
LiH
O3

A

3

116
Q

a chemical formula represents

qualitative info only
quantitative info only
both quantitative and qualitative info
neither info

A

3

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