WorksheetsElectrons and Periodic Table Review
Total questions: 40
Worksheet time: 1hrs 20mins
When an atom loses an electron, the atom becomes
an ion that is
negatively charged and its radial size increases
positively charged and its radial size increases
positively charged and its radial size decreases
negatively charged and its radial size
decreases
What is the total number of valence electrons in an
atom of germanium in the ground state?
8
32
14
4
Which atom in the ground state has an outermost
electron with the most energy?
Na
Rb
Li
Cs
The diagram represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of two of these elements.
Which two elements are in this mixture?
barium and hydrogen
helium and lithium
barium and lithium
helium and hydrogen
Electron X can change to a higher energy level or a
lower energy level. Which statement is true of
electron X?
Electron X neither emits nor absorbs energy
when it changes energy level.
Electron X absorbs energy when it changes to
a lower energy level.
Electron X emits energy when it changes to a
higher energy level.
Electron X absorbs energy when it changes to
a higher energy level.
Compared to a sodium atom in the ground state, a sodium atom in the excited state must have
a greater number of electrons
a smaller number of electrons
an electron with greater energy
an electron with less energy
What is the total number of kernel electrons in an atom of phosphorus in the ground state?
5
15
10
8
What is the total number of occupied principal energy levels in a neutral atom of neon in the ground state?
1
2
3
4
Given the electron configuration of an atom in the ground state: 2 - 8 - 6
This element is found in the Periodic Table in
Period 4 and Group 16
Period 4 and Group 14
Period 3 and Group 16
Period 3 and Group 14
In the ground state, atoms of which of the following elements have the highest first ionization energy?
boron
carbon
oxygen
nitrogen
As an atom in the excited state returns to the ground state, the energy of the atom
increases
decreases
remains the same
Which electron configuration represents an atom in an excited state?
2-6
2-7
2-7-1
2-8-1
Which is an electron configuration for an atom of chlorine in the excited state?
2-8-7
2-8-8
2-8-6-1
2-8-7-1
The characteristic bright-line spectrum of an element is produced when electrons
absorb energy and return to lower energy levels
absorb energy and move to higher energy levels
release energy and return to lower energy levels
release energy and move to higher energy levels
The electron-dot symbol X: would best represent
Na
Mg
Cl
Ne
Which Lewis electron-dot diagram represents a boron atom in the ground state?
Which atom has the weakest attraction for electrons in a chemical bond?
a boron atom
a calcium atom
a fluorine atom
a nitrogen atom
Which elements have the most similar chemical properties?
boron and carbon
oxygen and sulfur
aluminum and bromine
argon and hydrogen
Which represents the electron configuration of a metalloid in the ground state?
2-3
2-5
2-8-5
2-8-6
Which list of elements contains a metal, a metalloid, and a nonmetal?
Zn, Ga, Ge
Si, Ge, Sn
Cd, Sb, I
F, Cl, Br
Which element is brittle and does not conduct heat or electricity?
P(s)
Mg(s)
Al(s)
K(s)
At STP, what is the atomic number of the element that is solid, brittle, and a poor conductor of electricity?
12
13
16
17
Which set of properties is most characteristic of transition elements?
colorless ions in solution, multiple positive oxidation states
colorless ions in solution, multiple negative oxidation states
colored ions in solution, multiple positive oxidation states
colored ions in solution, multiple negative oxidation states
Oxygen and its allotrope ozone differ in the
number of atoms in the molecule.
number of protons in the nucleus.
number of principal energy levels.
number of neutrons in the nucleus.
At STP, which list consists entirely of diatomic molecules?
hydrogen, helium, fluorine, neon
oxygen, sulfur, selenium, tellurium
fluorine, chlorine, bromine, iodine
carbon, oxygen, nitrogen, bromine
In the Periodic Table, metallic character increases from
left to right and top to bottom
bottom to top of a group
bottom to top of a group, only
top to bottom of a group
The strength of an atom's attraction for the electrons in a chemical bond is the atom's
electronegativity
ionization energy
heat of reaction
ground state
Which of the following has the smallest ionic radius?
Mg2+
Ba2+
Ca2+
K+
Which statement correctly describes diamond and graphite, which are different forms of solid carbon?
They differ in their molecular structure,only.
They differ in their properties, only.
They differ in their molecular structure and properties.
They do not differ in their molecular structure or properties.
On the modern Periodic Table, the elements are arranged in order of increasing
atomic mass
atomic number
mass number
oxidation number
As the elements in Period 3 of the periodic table are considered from left to right, the degree of nonmetallic character of each successive element tends to
increases
decreases
remains the same
The periodic law states that the chemical properties of elements are periodic functions of their
density
atomic mass
atomic number
atomic radius
What occurs as the atomic number of the elements in Period 2 increases?
The nuclear charge of each successive atom decreases, and the atomic radius decreases.
The nuclear charge of each successive atom decreases, and the atomic radius increases.
The nuclear charge of each successive atom increases, and the atomic radius decreases.
The nuclear charge of each successive atom increases, and the atomic radius increases.
As the Group 1 elements of the Periodic Table are considered from top to bottom, the first ionization energy of each successive element decreases. One reason for this is that the
nuclear charge is decreasing
number of neutrons is increasing
number of principal energy levels is decreasing
distance between the valence electron and the nucleus is increasing
From the list below, which first ionization energy would indicate the most reactive metal?
500 kJ/mol
600 kJ/mol
700 kJ/mol
800 kJ/mol
Which atomic number represents an element that occurs only as compounds in nature because it is extremely reactive?
11
26
16
54
Which statement explains why neon is a group 18 element?
Neon is a gas at STP.
Neon has a low melting point.
Neon atoms have a stable valence electron configuration.
Neon atoms have two electrons in the first shell.
As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to
decreasing radius and decreasing shielding effect
decreasing radius and increasing shielding effect
increasing radius and decreasing shielding effect
increasing radius and increasing shielding effect
Based on Reference Table S, which of the following atoms requires the least energy for the removal of the most loosely bound electron?
Sn
Sr
Be
Br
Which electron transition represents a gain of energy?
from 2nd to 3rd shell
from 2nd to 1st shell
from 3rd to 2nd shell
from 3rd to 1st shell
