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WorksheetsF22 SE Review: Attraction
Total questions: 37
Worksheet time: 3hrs 33mins
What is ionization energy?
Energy needed to destroy an atom
Energy required to remove an electron from an atom in its gaseous state
Energy needed to split an electron
Energy associated with how strongly an atom attracts electrons
Electronegativity is...
the measure of how strongly an atom attracts electrons
the ability of an atom to lose electrons
the energy required to remove an electron from a specific atom in its gaseous state
how easy it is to make friends.
What is the atomic radius?
The distance from the nucleus to the outer boundary of an atom
The distance from one side of an atom to the other side
The distance around the atom
The distance between atoms in the gas phase
The distance between atoms in the solid phase
As you move across the periodic table atoms tend to get smaller because, ______________.
the atoms have more mass.
the atoms have less mass
the atoms have a bigger effective nuclear charge
the atoms have less electrons.
Which atom has the largest atomic radius?
potassium
rubidium
francium
cesium
The atom with the largest atomic radius in Group 18 is
Ar
He
Kr
Rn
Which of these has the largest atomic radius?
oxygen
fluorine
sulfur
chlorine
Which of these elements has the smallest atomic radius?
C
Ne
K
Al
P
Atomic radius generally increases as we move __________.
down a group and from right to left across a period
up a group and from left to right across a period
down a group and from left to right across a period
up a group and from right to left across a period
Which of the following will have a larger radius than zinc?
gallium
aluminum
magnesium
strontium
Order the following from smallest to largest atomic radius:
Ra, Be, Ca, Rb, H
Ra, Be, Rb, H, Ca
Rb, H, Ca, Be, Ra
Ra, Rb, Ca, Be, H
H, Be, Ca, Rb, Ra
The effective nuclear charge of magnesium is
+1
+2
+12
+24
Which one has the largest radius?
lithium
boron
neon
nitrogen
Effective nuclear charge ________ across a period.
increases
decreases
stays the same
Why does Cs have a larger radius than Na?
It has more energy levels
It has fewer energy levels
It has a more effective nuclear charge
It has a less effective nuclear charge
Why does Ca have a larger radius than Se?
It has more energy levels
It has fewer energy levels
It has a more effective nuclear charge
It has a less effective nuclear charge
Why is S smaller than Te?
It has more energy levels.
It has fewer energy levels.
It has a more effective nuclear charge.
It has a less effective nuclear charge.
What is effective nuclear charge?
The charge that effects the mass of the atom.
The charge that the protons feel from the rest of the atom.
The charge felt by the valence electrons.
The charge felt by the core electrons.
As you move down a group, the effective nuclear charge
increase
decreases
stays the same
Which of the following elements has the most "shielding" electrons?
nitrogen
phosphorus
arsenic
bismuth
In the following configuration, which electrons are the core electrons? 1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6
3s2 3p4
1s2 2s2
2s2 2p6 3s2 3p4
increase
decreases
stays the same
What is the electron Configuration of Lithium
1s12s1
1s222
1s22s1
1s12s2
What element has a configuration of 1s2 2s2 2p2 ?
Carbon
Oxygen
Fluorine
Nitrogen
What is the electron configuration of Magnesium?
1s22s22p63s1
1s22s22p6
1s22s22p63s2
1s22s22p6
What element is represented by this PES graph?
Aluminum
Nitrogen
Chlorine
Phosphorus
What is electron shielding?
Inner electrons shield the valence shell from protons
Valence electrons shield the inner electrons from atoms
Electrons build an impenetrable shield against neutrons
Electrons are used to shield a radioactive isotope
Which element has the most electron shielding?
O
S
Cu
Se
Which electrons are responsible for shielding?
Valence electron
Core electrons
s- and p- orbital electrons
All electrons in the atom
Shielding increases with ...
a decreasing number of energy levels
an increasing number of energy levels
an increasing number of valence electrons
a decreasing number of valence electrons
