NEW
Font size
WorksheetsPre-UPS3 Periodic Table
Total questions: 20
Worksheet time: 20mins
As you move down the periodic table, size of atoms get bigger. This is because ____________.
shielding effect increases
effective nuclear charge decrease
proton number increases
nucleus attraction towards valence electrons increases
As you move across the periodic table atoms tend to get smaller because, ______________.
proton number decreases
effective nuclear charge increases
shielding effect decreases
nucleus attraction towards valence electrons decreases
Which statement correctly and completely identifies a trend?
Atomic radius decreases across a period and increases down a group.
Electronegativity decreases across a period and decreases down a group.
First ionization energy increases across a period and increases down a group.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
Sodium is more electronegative than potassium.
Sodium has more energy levels than potassium.
Sodium has a larger atomic radius than potassium.
Sodium has lower ionization energy than potassium.
Which of the following atoms has the smallest atomic radius?
O
B
C
F
Choose the correct statement.
The size of atoms will increase from left to right because the increasing number of electrons occupy more space creating a larger atom.
The size of atoms will increase from left to right because the increasing number of electrons tends to overcome the pull of the protons and increase the size of their orbitals
The size of atoms will decrease from left to right because the increasing number of electrons are adding mass to the outside which is pulled toward the center.
The size of atoms will decrease from left to right because the increasing number of protons results in a greater pull on the electrons toward the nucleus.
Electronegativity is...
the ability of an atom to attract/ accept electrons
the ability of an atom to lose electrons
the energy required to remove an electron from a specific atom
the ability of an atom to remove electrons
Ionization energy is...
the energy required to add an electron to a specific atom
the energy required to remove an electron from an atom
the energy required to shield the outer electrons from the nucleus
a measure of the ability of an atom to attract electrons
Which statement correctly and completely identifies a trend?
Atomic radius increases across a period and increases down a group.
Electronegativity increases across a period and decreases down a group.
Ionization energy decreases across a period and increases down a group.
Electronegativity decreases across a period and increases down a group.
Energy level increases when going down a group of the periodic table. Increases of energy levels lead to
electron shielding and a larger atomic radius
electron shielding and a smaller atomic radius
electron shielding and a higher ionization energy
electron shielding and a higher electronegativity value
When comparing the size of O atom and O2- ion which of the following statements is true?
O2- ion is smaller than O atom
The electron-electron repulsion in O2- ion is higher than O atom
Two electrons are removed from O atom to form O2- ion.
O2- ion has more protons than O atom
When comparing the size of Li atom and Li+ ion which of the following statements is false?
Li+ ion is smaller than Li atom
One electron is removed from Li atom to form Li+ ion.
The electron-electron repulsion in Li+ ion is higher than in Li atoms.
Li atom and Li+ ion have the same number of protons.
Which of these has the larger atomic radius?
B
Li
N
O
What causes the shielding effect to remain constant across a period?
The atomic radius increases
The charge on the nucleus is constant.
Electrons are added to the same principal energy level.
Electrons are added to different principal energy levels.
Element Q has the following electronic configuration:
1s2 2s2 2p6 3s2 3p6 3d5 4s1
Which of the following is true about the position of element Q in periodic table?
Period 3, Group 1, Block s
Period 4, Group 16, Block d
Period 4, Group 6, Block d
Period 4, Group 1, Block s
The higher the ionization energy...
the more attracted the valence electron is to the nucleus
the less attracted the valence electron is to the nucleus
the more attracted the valence electron is to another electron
the less attracted the valence electron is to another electron
In general, as you go across a period in the periodic table from left to right:
(1) the atomic radius __________;
(2) the electronegativity __________; and
(3) the first ionization energy __________.
decreases, decreases, increases
increases, increases, decreases
increases, increases, increases
decreases, increases, increases
The ionization energy of nitrogen is more than that of oxygen because
Nitrogen has stable half filled p-orbitals
Nitrogen is left to the oxygen in the same period of the periodic table
Nitrogen contains less number of electrons
Nitrogen is less electronegative
Magnesium is in group 2 in the periodic table. Which of the following formulas for magnesium
compounds is correct?
MgO2
MgS2
MgF2
Mg2O
Which factor contributes to the increase in radius down a group?
Increase size of nucleus
fewer electrons in higher energy levels
shielding of inner electrons
increase in protons
