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