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Chemistry Midterm
Chemistry Midterm
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#chemistry #science #grade_10
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1
The gold foil experiment led to the discovery of the
neutron
electron
cathode ray
nucleus
2
The carbon-12 atom is assigned a relative mass of exactly
12 amu
6 amu
100 amu
1 amu.
3
From gaps in his table, Mendeleev predicted the existence of several elements and their
atomic numbers
properties
colors
radioactivity
4
which of the following is not a SI base unit
liter
kilogram
kelvin
second
5
Isotopes are atoms of the same element that have different
numbers of electrons.
principal chemical properties.
masses.
numbers of protons.
6
To which group of hte periodic table do fluorine and chlorine belong
transition elements
halogens
actinides
alkaline-earth metals
7
To which group of the periodic table do lithium and potassium belong?
noble gases
hlaogens
alkali metals
transition metals
8
When applied ot scientific measurements, the words accuracy and precision
are used interchangeably.
have distinctly different meanings.
can cause uncertainty in experiments.
have limitations.
9
Who explained the behavior of positively charged particles being deflected from a metal foil as the nucleus
John Dalton
James Chadwick
Ernest Rutherford
Niels Bohr
10
the number of significant figure in the measurement 170.040 km is
5
3
4
6
11
Trends in the periodic table indicate that the element with the most ionization energy is in which periods and groups
Period 7, Group 2
Period 2, Group 1
Period 1, Group 18
Period 6, Group 17
12
The law of conservation of mass follows from the concept that
atoms of different elements have different properties.
atoms can be destroyed in chemical reactions.
atoms are indivisible.
matter is composed of atoms.
13
The process that changes one element into another different element is called
transformation.
transfiguration.
transgeneration
transmutation.
14
The number of orbitals for the d sublevel is
7
1.
3
5
15
I the gold foil experiment, most of the particles fired at the foil
bounced back.
combined with the foil.
passed through the foil.
were absorbed by the foil.
16
The letter designations for the four sublevels, with the number of electrons that can be held in each sublevel are
s: 1, p: 2, d: 3, and f: 4
s: 2, p: ,6 d: 10, and f: 14.
s: 1, p: 3, d: 5 and f.7
s: 1, p: 3, d: 10, and f: 14.
17
The composition of the two oxides of lead, PbO and PbO2 are explained by the
atomic law
periodic law
law of conservation of mass
law of multiple proportions
18
According to Dalton's atomic theory, atoms
can be divided.
of different elements cannot combine.
are destroyed ni chemical reactions
of each element are identical ni size, mass, and other properties.
19
the abbreviation that represents a volume unit is
mg
mL
mm
cm
20
The state of matter in which a material has neither a definite shape nor a definite volume is the state
liquid
solid
gaseous
elemental
21
Five darts strike near the center of the target. Whoever threw the darts is
both accurate and precise.
precise.
accurate.
neither accurate nor precise.
22
The idea of arranging the elements ni a table according ot their chemical and physical properties is attributed to
Newlands
Bohr
Moseley
Ramsay
23
all of the following are examples of units except
weight
gram
teaspoon
kilometer
24
A measure of the quantity of matter is
density
volume
mass
weight
25
A chemical change occurs when
salt deposits form from evaporated seawater.
a leaf changes color.
dissolved minerals solidify to form a crystal.
ethanol si purified through distillation.
26
The mass of a neutron is
about the same as that of a proton.
double that of an electron.
double that of a proton.
about the same as that of an electron.
27
Bohr's theory helped explain why
electrons have negative charge.
excited hydrogen gas gives off certain colors of light.
atoms combine to form molecules.
most of the mass of the atom is in the nucleus
28
Protons and neutrons strongly attract when they
have opposite charges.
are moving fast
are at high energies.
are very close together.
29
The elements in Group 17 are known by what name?
halogens
alkali metal
noble gases
alkaline earth metals
30
The sequence ni which energy sublevels are filed is specified by
aufbau principle.
the Pauli exclusion principle.
Lyman's series.
the orbital rule.
31
A chemist who frequently carries out a complex experiment is likely to have high
accuracy
accuracy, but low precision.
precision, but low accuracy.
precision
32
"Orbitals of equal energy each get one electron before any gets a second electron" is a statement of
the quantum effect
Hund's rule.
the Pauli exclusion principle.
the aufbau principle
33
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
the Pauli exclusion principle
Hund's rule
the Pauli exclusion principle
the aufbau principle.
34
The outer electron configuration of an alkali metal has
2 electrons in the s orbital.
2 electrons in the p orbital
1 electron in the s orbital
1 electron in the p orbital.
35
A solution of two or more metals is
a jelly
an insulator.
brittle
an alloy.
36
A chemical formula for a molecular compound represents the composition of
the crystal lattice
a molecule.
an ato,
the ions that make up the compound.
37
Isotopes of an element contain different numbers of
protons
neutrons
nuclides
electrons
38
Most of the volume of an atom is occupied by the
protons
nucleus.
nuclides.
electron cloud.
39
Matter includes al of the following except
vapor
air
smoke
light
40
When the light from excited atoms of na element is passed through a prism the distinct colored lines produced are called
ground states
excited states
line-emission spectra
electromagnetic spectra
41
the SI base unit for time is the
second
hour
minute
day
42
to calculate the density of an object
divide its mass by its area
multiply its mass and its volume
divide its volume by its mass
divide its mass by its volume
43
Which of the following is NOT part of Dalton's atomic theory?
The number of protons in an atom is its atomic number.
All matter is composed of extremely small particles called atoms.
In chemical reactions, atoms are combined, separated, or rearranged.
Atoms cannot be divided, created, or destroyed
44
A metal is called malleable if it
can be squeezed out into a wire.
has a shiny appearance.
exists naturally as an element._
can be hammered into sheets
45
Mendeleev is credited with developing the first successful
test for radioactivity
periodic table
use of X rays
method for determining atomic number
46
The statement that no more than two electrons in the same atom can occupy a single orbital is
Bohr's law
Hund's rule.
the ayfbua principle
the Pauli exclusion principle.
47
What did Rutherford conclude about hte structure of the atom?
Electrons make up hte center of an atom.
An atom contains a small, dense, positively charged central region.
An atom carries apositive charge.
An atom is indivisible.
48
Going dow a group in the periodic table, electron sheilding generally causes the effective nuclear charge to
increase
vary unpredictably
remain the same
decrease
49
When density si measured,
the temperature should be specified.
the mass and volume do not need to be measured._ 19.
a balance is always used.
the units are always kg/m3
50
Atoms of the same element that have different masses are caled
moles.
isotopes
nueutrons
nuclides
51
which of the following does not describe a measurement standard
measurement standards avoid ambiguity
confusion is eliminated when the correct measurement standard is applied
a standard need not agree with previously defined size
measurement standards most be unchanging
52
An element in which of the following periods and groups will have the smallest anion (negative ion) radius
Period 2, Group 1
Period 4, Group 16
Period 1, Group 17
period 7, Group 2
53
In division and multiplication, the answer must not have more significant figures than the
total number of significant figures ni the calculation.
number ni the calculation with the fewest sign
average number of significant figures in the calculation.
number in the calculation with the most significant figures.
54
"In any chemical or physical process, energy is neither created nor destroyed" is a statement of the
system
law of conservation of energy.
law of physical and chemical change.
law of conservation of mass.
55
When determining the number of significant digits in a measurement,
all zeros between two nonzero digits are not significant.
all nonzero digits are significant.
all zeros are significant.
all nonzero digits are not significant.
56
Moving from left to right across _ electrons are being added to the 4f orbitals
the noble gases
the lanthanides
the halogens
period 4
57
The principle that states that the properties of the elements are periodic functions of their atomic numbers is
the periodic law.
the periodic table.
the law of properties.
Mendeleev's law.
58
A method of measuring the size of an atom where a value that is _ the distance between the nuclei of two bonded atoms.
half
one-quarter
twice
equal to
59
A property of all actinides is that they are
nonmetals.
Both (a) and (b)
members of Period 7
radioactive.
60
Under ordinary conditions of temperature and pressure, the particles in a gas are
held in fixed positions.
very far from each other.
closely packed
unevenly distributed.
61
I electrons ni an atom have the lowest possible energies, the electrons are ni their
radiation-emitting states.
ground states.
excited states.
inert states.
62
In a cathode tube, electrical current passes from one electrode, the_ to the oppositely charged electrode.
both a and c
a cathode
c negatively charged electrode
b anode
63
The main energy levels of an atom are indicated by the
orbital quantum numbers.
spin quantum numbers.
principal quantum numbers.
magnetic quantum numbers
64
the relationship between the mass (m) of a material, its volume (V), and it's density(D)
DV=m
D+V=m
V=mD
Vm=d
65
the SI base unit for mass is the
second
gram
meter
kilogram
66
The law of definite proportions
assumes that atoms of all elements are identical.
replaced the law of conservation of mass
contradicted Dalton's atomic theory.
was explained by Dalton's atomic theory.
67
Transition elements are found in which of the following group(s) of the periodic table?
groups 3-12
group 1
groups 1 and 2
group 18
68
The periodic law states that
chemical properties can be grouped by periodicity physical properties cant
the properties of the elements are functions of their atomic numbers.
no two electrons with the same spin are in the same place in an atom
electrons exhibit properties of both particles and waves
69
According ot Bohr's theory, an excited atom would
produce line-emission spectra
collapse
radiate energy.
absorb photons
70
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a new octet forms
The number of energy levels increases.
The number of neutrons increases.
the nuclear charge increases
71
For an electron in an atom to change from the ground state to an excited state
the electron must make a transition from a higher ot a lower energy level.
radiation must be emitted
energy must be absorbed.
energy must be released.
72
1 cubic centimeter is equivalent to
10-1 cubic decimeters
1 liter
1 milileter
1 gram
73
A nuclear particle that has about the same mass as a proton, but with on electrical charge, is called a(n)
nuclide.
isotope
neutron
electron
74
To two significant figures, the measurement 0.0255 g should be reported as
0.02 g
0.025 g
2.5\times10^2 g
0.026 g
75
An aluminum isotope consists of 31 protons, 31 electrons, and 41 neutrons. Its mass number is
14
27
13
40
76
Which part of an atom has a mass approximately equal ot 1/2000 of the mass of a common hydrogen atom?
nucleus
proton
electron
electron cloud
77
Elements in a group have similar
reactivities
electron configurations
symbols
densities
78
Quantitive observations are recorded using
non-numerical information
numerical information
a system
a control
79
Going across a period in the periodic table, electron shielding has little effect so, the effective nuclear charge
increases
remain the same
decreases
varies unpredictably
80
The atomic number of na, the first element in Period 3, is 11. The atomic number of the second element in this period is
10
12
3
18
81
A physical change occurs when a
copper bowl tarnishes.
glue gun melts a glue stick.
bracelet turns your wrist green.
peach spoils.
82
the abbreviation for mm represents
meter
millimeter
micrometer
milliliter
83
Who first proposed an atomic theory based on scientific knowledge?
Dmitri Mendeleev
Robert Brown
Jons Berzelius
John Dalton
84
For every investigation, the scientific method
is the same set of procedures
is a logical set of procedures.
must be abandoned fi there are unexpected results
helps to predict what results will be obtained
85
the liter is defined as
1000g3
1000 cm3
1000 c3
1000 m3
86
Elements in a group or column in the periodic table can be expected to have similar
properties
atomic numbers.
atomic masses
numbers of neutrons.
87
The energy that results from the breaking or formation of chemical bonds is
temperature
kinetic energy
potential energy
chemical energy
88
The effect of inner electrons on the attraction between the nucleus and the outer electrons of an atom is called
electronegativity.
electron affinity
electron shielding.
electron ionization
89
Trends in the properties of elements in a group or period can be explained in terms of
electron affinity
atomic number.
binding energy.
electron configuration.
90
Nitrogen monoxide and oxygen 2 clear gases, form a red-brown gas when mixed. Nitrogen monoxide and oxygen are called the
products.
equilibria
reactants
synthetics
91
Which of the following rules requires that each of the p orbitals receive one electron before any of them can get more
the Pauli exclusion principle
Hund's rule
the aufbau principle
the quantum rule
92
The nucleus of most atoms is composed of
tightly packed neutrons.
loosely connected protons and electrons.
tightly packed protons and neutrons
tightly packed protons.
93
Experiments with cathode rays led ot the discovery of the
proton
electron
nucleus
neutron
94
which of the following does not describe a unti
a unit compares what is being measured with a previously defined size
a unit is usually preceded by a number
the choice of a unit depends on the quantity being measured
a unit is not needed to find a solution to a problem
95
Electron affinity tends to
increase across a period and increase down a group.
decrease across a period and increase down a group.
increase across a period and decrease down a group.
decrease across a period and decrease down a group.
96
The measurement that has been expressed to four significant figures is
0.00402 mm
402.10 mm
30.00 mm
0.0020 mm
97
The abbreviation for atomic mass unit is
amu
a
u
mu
98
Precision pertains to all of the folowing except
reproducibility of measurements
agreement among numerical values.
closeness of a measurement to an accepted value.
sameness of measurements.
99
an element ni which of the following periods and groups will have the largest cation (positive ion) radius
Period 2, group 2
Period 4, Group 2
Period 7, Group 1
Period 1, Group 17
100
The statement that an electron occupies the lowest available energy orbital is
Bohr's law
the Pauli exclusion principle.
the aufbau principle.
Hund's rule.
