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WorksheetsUnit 3 Formative Assessment
Total questions: 20
Worksheet time: 10mins
Name
Class
Date
1.
What are the three broad classes of elements shown on the periodic table?
a)
Solids, liquids, gasses
b)
metals, nonmetals, gasses
c)
metals, liquids, noble gasses
d)
metals, nonmetals, metalloids
2.
Which elements are examples of nonmetals?
a)
sodium, potassium, calcium
b)
silicon, germanium, astanine
c)
barium, iron, cobalt
d)
argon, sulfur, oxygen
3.
Which two elements have properties most similar to those of the element Sodium?
a)
lithium, potassium
b)
magnesium, aluminum
c)
selenium, scandium
d)
krypton, zenon
4.
How many electrons are in the highest occupied energy level of an element in Group 5A (Group 15)?
a)
1
b)
3
c)
5
d)
7
5.
As shown by the periodic table, why do the elements potassium and sodium have similar chemical properties?
a)
They are in the same group and have the same number of electrons in the highest occupied energy level
b)
They are in the same group and an atom of either element has one electron in a p orbital.
c)
They are in the same period and an atom of either element has an odd number of protons in its nucleus.
d)
They are in the same period and a sodium atom has only one more electron than a potassium atom has.
6.
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a)
Pt
b)
V
c)
Li
d)
Kr
7.
The electron configuration for an element is 1s22s22p63s23p6. What is the atomic number of the element?
a)
3
b)
11
c)
18
d)
22
8.
Iron is a transition metal with an atomic number of 26. What is the electron configuration of iron?
a)
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6
b)
1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 4s^2
c)
1s^2 2s^2 2p^6 3s^2 3p^6 3d^8
d)
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^6
9.
Use your understanding of the experimental design and conclusions used in the development of modern atomic theory to answer this question: What was Bohr's basic proposal about the atom?
a)
An electron remains in a fixed position in the space around the nucleus.
b)
An electron is found in a specific circular path, or orbit, around the nucleus.
c)
An electron oscillates, or moves back and forth, within one small region of space in the atom.
d)
An electron readily exchanges position with either a proton or a neutron
10.
Which is NOT one of the three rules for writing the electron configurations of elements?
a)
Aufbau Principle
b)
Pauli Exclusion Principle
c)
Law of Conservation of Energy
d)
Hund's Rule
11.
How does the energy of an electron change when the electron moves closer to the nucleus?
a)
decreases
b)
increases
c)
does not change
d)
doubles
12.
The isotopes hydrogen-1 and hydrogen-2 make up nearly all of the hydrogen found in nature. The mass of an atom of hydrogen-1 is 1.0078 amu, and the mass of an atom of hydrogen-2 is 2.0141 amu. Because the atomic mass of hydrogen is 1.0079 amu, what can be concluded about the two isotopes?
a)
Hydrogen-1 is by far the more abundant isotope.
b)
Hydrogen-2 is by far the more abundant isotope.
c)
Hydrogen-1 and hydrogen-2 are about equally abundant.
d)
The isotope hydrogen-3 does not exist in nature.
13.
What are three types of subatomic particles?
a)
Ions, neutrons, nucleus
b)
Protons, electrons, nucleus
c)
Muons, ions, electrons
d)
Protons, electrons, neutrons
14.
What distinguishes the atoms of one element from the atoms of another?
a)
The number of protons in the nucleus
b)
The number of neutrons in the nucleus
c)
The total number of protons and neutrons in the nucleus
d)
The total number of protons, neutrons, and electrons
15.
How do the isotopes of a given element differ from one another?
a)
They have the same mass numbers but different numbers of protons
b)
They have the same mass numbers but different numbers of electrons.
c)
They have different mass numbers and different numbers of neutrons.
d)
They have different mass numbers and the electrons of the atoms are arranged in different ways.
16.
What are the relative charges of the three main subatomic particles?
a)
Proton 1+, electron 1–, neutron 1+
b)
Proton 1+, electron 1–, neutron 0
c)
Proton 2+, electron 1–, neutron 0
d)
Proton 2+, electron 1+, neutron 1–
17.
The nucleus of an atom is
a)
the central core and is composed of protons and neutrons.
b)
positively charged and has more protons than neutrons
c)
negatively charged and has a high density.
d)
negatively charged and has a low density.
18.
What is this element and how many valence electrons does is possess?
a)
Oxygen; 5
b)
Oxygen; 6
c)
Phosphorus; 5
d)
Nitrogen; 5
19.
In what order is the periodic table arranged?
a)
Number of neutrons
b)
Number of electrons
c)
Atomic mass
d)
Number of protons
20.
What does this image tell us?
a)
Bromine has an atomic number of 7
b)
Boron has 7 valence electrons
c)
Boron has 7 electrons
d)
Bromine has 7 valence electrons
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