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WorksheetsAtomic Structure Honors
Total questions: 25
Worksheet time: 27mins
Name
Class
Date
1.
Chlorine has atomic # 17 and mass # 35. It has
a)
17 protons, 17 electrons and 18 neutrons
b)
35 protons, 35 electrons and 17 neutrons
c)
17 protons, 17 electrons and 52 neutrons
d)
18 protons, 18 electrons and 17 neutrons
2.
If two or more compounds are composed of the same two elements, the ratio of the masses of one element that combine with a fixed mass of the other element is a simple whole number. This is a statement of the law of
a)
conservation of mass
b)
mass action
c)
multiple proportions
d)
definite composition
3.
The rays produced in a cathode tube are
a)
unaffected by a magnetic field
b)
deflected away from a negative plate
c)
found to carry a positive charge
d)
striking the cathode
4.
The average atomic mass of an element is the average of the atomic masses of its
a)
naturally occurring isotopes
b)
two most abundant isotopes
c)
radioactive isotopes
d)
artificial isotopes
5.
According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a)
equal to
b)
greater than
c)
less than
d)
either greater than or less than
6.
Which concept in Dalton's atomic theory has been modified?
a)
all matter is composed of atoms
b)
atoms of different elements have different properties and masses
c)
atoms can combine in chemical reactions
d)
atoms cannot be divided
7.
In determining the atomic mass of elements, the standard is the
a)
C-12 atom
b)
C-14 atom
c)
H-1 atom
d)
O-16 atom
8.
In Rutherford's experiments, most of the particles
a)
bounced back
b)
passed through the foil
c)
were absorbed by the foil
d)
combined with the foil
9.
Whose series of experiments identified the nucleus of the atom?
a)
Rutherford
b)
Dalton
c)
Chadwick
d)
Bohr
10.
In oxides of nitrogen, such as N2O, NO, NO2, and N2O3, atoms combine in small whole-number ratios. This evidence supports the law of
a)
conservation of mass
b)
multiple proportions
c)
definite composition
d)
mass action
11.
The principles of atomic theory recognized today were conceived by
a)
Avogadro
b)
Bohr
c)
Dalton
d)
Rutherford
12.
Dalton incorporated the law of conservation of mass into his atomic theory by asserting that
a)
atoms are indivisible
b)
atoms of different elements have different properties
c)
matter is composed of atoms
d)
atoms can be destroyed in chemical reactions
13.
Neon-22 contains 12 neutrons. It also contains
a)
12 protons
b)
22 protons
c)
22 electrons
d)
10 protons
14.
An atom is electrically neutral because
a)
neutrons balance the protons and electrons
b)
nuclear forces stabilize the charges
c)
the numbers of protons and electrons are equal
d)
the number of protons and neutrons are equal
15.
The total number of protons and neutrons in the nucleus of an atom is its
a)
atomic number
b)
Avogadro number
c)
mass number
d)
average atomic mass
16.
The atomic theory proposed by Dalton has been
a)
totally discarded
b)
expanded and modified
c)
accepted unchanged to the present day
d)
found to be plagiarized
17.
The radius of an atom extends to the outer edge of the
a)
nucleus
b)
region occupied by the electrons
c)
region occupied by the neutrons
d)
positive charges
18.
Nuclear forces exists because the particles in the nucleus are
a)
oppositely charged
b)
close together
c)
highly energized
d)
moving very fast
19.
All isotopes of hydrogen contain
a)
one neutron
b)
two electrons
c)
one proton
d)
two nuclei
20.
Most of the volume of an atom is occupied by the
a)
nucleus
b)
nuclides
c)
electrons
d)
protons
21.
As the mass number of an element's isotopes increases, the number of protons
a)
decreases
b)
increases
c)
doubles each time the mass number increases
d)
remains the same
22.
The number of atoms in 1 mol of carbon is
a)
6.022 × 1022
b)
6.022 x 1023
c)
5.022 x 1022
d)
5.022 x 1023
23.
If 4.0 g of element A combine with 10. g of element B, then 12 g of element A combine with ____ g of element B.
a)
10
b)
12
c)
24
d)
30
24.
Determine the mass in grams of 5.00 mol of oxygen. The molar mass of bromine is 16.0 g/mol.
a)
.313 g O
b)
8.30 x 10-24 g O
c)
80.0 g O
d)
3.01 x 1024 g O
25.
Calculate the number of atoms in 10.0 g of sulfur (molar mass 32.07 g/mol).
a)
5.33 x 10-22 atoms S
b)
1.88 x 1023 atoms S
c)
1.93 x 1026 atoms S
d)
5.19 x 10-25 atoms S
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