WorksheetsThe Periodic Table
Total questions: 52
Worksheet time: 26mins
Which list of elements consists of a metal, a metalloid, and a nonmetal?
Si, F, Mg
H, Na, Cl
Al, Cu, Ne
Ge, As, K
Which characteristics both generally decrease from left to right across Period 3?
Nonmetallic properties and atomic radius
Nonmetallic properties and ionization energy
Metallic properties and atomic radius
Metallic properties and ionization energy
As the elements in Group 17 are considered in order of increasing atomic number, the chemical reactivity of each successive element
increases
decreases
remains the same
As the elements in Group 1 are considered in order of increasing atomic number, the chemical reactivity of each successive element
increases
decreases
remains the same
Elements on the most current periodic table are arranged based on
increasing atomic number
electron configuration
both of above
neither of above
Which phrase best describes the elements in Group 2 of the Periodic Table?
Group 2 is classified as metals and called the Alkaline earth metals
Group 2 is classified as metalloids and called Alkali metals
Group 2 is classified as metals and called Transition metals
Group 2 is classified as nonmetals and called Halogens
Which phrase best describes the elements in Group 1 of the Periodic Table?
Group 1 is classified as metals and called the Alkaline earth metals
Group 1 is classified as metalloids and called Alkali metals
Group 1 is classified as metals and called Alkali metals
Group 1 is classified as nonmetals and called Halogens
Which phrase best describes the elements in Group 17 of the Periodic Table?
Group 17 is classified as metals and called the Alkaline earth metals
Group 17 is classified as metalloids and called Alkali metals
Group 17 is classified as metals and called Alkali metals
Group 17 is classified as nonmetals and called Halogens
Which list includes elements with the most similar chemical properties?
O, C, N
O, S, Se
Na, Mg, Al
Na, F, Ne
What are valence electrons?
Subatomic particles that are found in the nucleus of the atom.
Subatomic particles that are outside of the nucleus.
Subatomic particles that are found in space.
Subatomic particles that are found in the outermost energy level.
A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a
metal
metalloid
noble gas
nonmeta;
An element that has a low first ionization and good conductivity of heat and electricity is classified as a
metal
metalloid
noble gas
nonmeta;
Which element has chemical properties that are most similar to the chemical properties of chlorine?
S
Ar
P
F
Which element is solid, brittle, and a poor conductor of electricity?
iodine
potassium
hydrogen
neon
Which statement explains why argon 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
An atom of neon in the ground state tends not to bond with an atom of a different element because the neon atom has
More protons than neutrons
More neutrons than protons
A total of two valence electrons
A total of eight valence electrons
Which Group 14 element is a metalloid?
tin
lead
silicon
carbon
What is the total number of valence electrons in a lead atom in the ground state?
22
2
32
4
What is the total number of valence electrons in a strontium atom in the ground state?
22
2
32
4
Oxygen and sulfur have similar chemical properties because an oxygen atom and a sulfur atom have the same
Atomic number
Mass number
Total number of electron shells
Total number of valence electrons
As the elements in Period 3 are considered in order of increasing atomic number, there is a general increase in all of the following except
atomic number
atomic radius
electronegativity
ionization energy
Which general trend is found in Period 3 as the elements are considered in order of increasing atomic number?
decreasing atomic mass
increaseing atomic radius
decreasing ionization energy
increasing elecronegativity
Which atom in the ground state requires the least amount of energy to remove its valence electron?
lithium
sodium
potassium
rubidium
Which atom in the ground state requires the least amount of energy to remove one valence electron?
sodium
magnesium
aluminum
silicon
Which element forms an ion that is larger than its atom?
potassium
calcium
gallium
bromine
As you read left to right across a period, the atomic radius of the elements generally
increase.
decrease.
double.
remains the same.
As you read left to right across a period, why does the atomic radius of the elements generally change the way it does?
increasing numbers of protons causes more nuclear pull, making atoms larger.
increasing numbers of protons causes less nuclear pull, making atoms smaller.
increasing numbers of protons causes more nuclear pull, making atoms smaller.
increasing numbers of protons causes less nuclear pull, making atoms larger.
Which element has the greatest electronegativity value?
Fr
Li
F
Rn
What does electronegativity mean?
an atom's ability to attract electrons to itself
energy required to remove an electron from an atom
energy released when an electron is added to an atom
force of attraction between the protons and electrons in an atom
What does electron affinity mean?
an atom's ability to attract electrons to itself
energy required to remove an electron from an atom
energy released when an electron is added to an atom
force of attraction between the protons and electrons in an atom
What does ionization energy mean?
an atom's ability to attract electrons to itself
energy required to remove an electron from an atom
energy released when an electron is added to an atom
force of attraction between the protons and electrons in an atom
What does Coulombic attraction mean?
an atom's ability to attract electrons to itself
energy required to remove an electron from an atom
energy released when an electron is added to an atom
force of attraction between the protons and electrons in an atom
A Period on the periodic table is
a vertical column of elements
a horizontal row of elements
A Group on the periodic table is
a vertical column of elements
a horizontal row of elements
Which statement is true about Coulombic Force?
Force of attraction increases between protons and electrons as distance increases
Force of attraction decreases between protons and electrons as distance increases
Force of attraction increases between protons and electrons as number of electrons increases
Force of attraction decreases between protons and electrons as number of electrons increases
Which statement is true about Coulombic Force?
Force of attraction increases between protons and electrons as distance increases
Force of attraction decreases between protons and electrons as distance decreases
Force of attraction increases between protons and electrons as number of protons increases
Force of attraction decreases between protons and electrons as number of protons increases
What is the trend in ionization energy across a period?
Ionization energy decreases because electrons are less attracted to increasing proton number
Ionization energy increases because electrons are more attracted to increasing proton number
Ionization energy decreases because electrons are further away from the nucleus due to added energy levels
Ionization energy decreases because electrons are further away from the nucleus due to added energy levels
What is the trend in ionization energy down a group?
Ionization energy decreases because electrons are less attracted to increasing proton number
Ionization energy increases because electrons are more attracted to increasing proton number
Ionization energy decreases because electrons are further away from the nucleus due to increased energy levels
Ionization energy decreases because electrons are further away from the nucleus due to increased energy levels
How many valence electrons do the elements in Group 15 have?
15
5
3
8
The number of rows on the periodic table is the same as the number of
occupied orbitals in the outer energy level.
electrons in an atom of that element.
valence electrons.
the energy level of the valence electrons.
What is the trend in electron affinity across a period?
Electron affinity decreases across a period because more energy levels are being added.
Electron affinity increases across a period because more energy levels are being added.
Electron affinity increases across a period because increased protons are pulling electrons with greater Coulombic force
Electron affinity decreases across a period because decreased protons are pulling with less Coulombic force
What is the trend in electron affinity down a group?
Electron affinity decreases down a group because more energy levels are being added.
Electron affinity increases down a group because more energy levels are being added.
Electron affinity increases down a group because increased protons are pulling electrons with greater Coulombic force
Electron affinity decreases down a group because decreased protons are pulling with less Coulombic force
What is the trend in electronegativity down a group?
Electronegativity decreases down a group because more energy levels are being added so there is less pull from the nucleus
Electronegativity increases down a group because more energy levels are being added so there is less pull from the nucleus
Electronegativity decreases down a group because fewer protons in the nucleus means less pull on the electrons
Electronegativity increases down a group more protons in the nucleus means more pull on the electrons
What is the trend in electronegativity across a period?
Electronegativity decreases across a period because more energy levels are being added so there is less attraction for electrons
Electronegativity increases across a period because more energy levels are being added so there is less attraction for electrons
Electronegativity decreases across a period because fewer protons in the nucleus means less attraction for electrons
Electronegativity increases across a period because more protons in the nucleus means more attraction for electrons
What is the trend in atomic radius as you move from left to right across a period?
atomic radius tends to increase as more energy levels are added
atomic radius tends to increase as more protons are added, pulling electrons closer
atomic radius tends to decrease as more electrons are added, spreading electrons further appart
atomic radius tends to decrease as more protons are added, pulling electrons closer
What is the trend in atomic radius as you move down a group?
atomic radius tends to increase as more energy levels are added
atomic radius tends to increase as more protons are added, pulling electrons closer
atomic radius tends to decrease as more electrons are added, spreading electrons further appart
atomic radius tends to decrease as more protons are added, pulling electrons closer
What is the trend in ionic size compared to atoms down a group?
metal ions tend to be smaller than metal atoms
metal ions tend to be larger than metal atoms
nonmetal ions tend to be smaller than nonmetal atoms
nonmetal atoms tend to be larger than nonmetal ions
What is the trend in ionic size compared to atoms down a group?
metal atoms tend to be smaller than metal ions
metal ions tend to be larger than metal atoms
nonmetal ions tend to be smaller than nonmetal atoms
nonmetal ions tend to be larger than nonmetal atoms
What is a cation?
a positively charged ion
a negatively charged ion
What is an anion?
a positively charged ion
a negatively charged ion
What is the trend in metallic character across a period?
metallic character tends to decrease
metallic character tends to increase
What is the trend in metallic character down a group?
metallic character tends to decrease
metallic character tends to increase
