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WorksheetsCH301 - Unit 1 Exam 2 Review
Total questions: 40
Worksheet time: 2hrs 44mins
The atom having the valence-shell configuration 4s2 4p5 would be in:
Group VIA and Period 5
Group IVB and Period 4
Group VIB and Period 7
Group VIIA and Period 4
Group VIIB and Period 4
Select the term best describing the series of elements: Mn, Fe, Co, Ni, Cu.
d-transition metals
main group elements
metalloids
alkaline earth metals
halogens
Which element has the largest atomic radius?
Li
Na
Rb
F
I
Which of the following terms accurately describes the energy associated with the process:
electron affinity
binding energy
ionization energy
electronegativity
none of these
Which element has the lowest first ionization energy?
He
Ne
Ar
Kr
Xe
Which element has the highest first ionization energy?
Be
B
C
N
O
Which of these isoelectronic species has the smallest radius?
Br-
Sr2+
Rb+
Se2-
They are all the same size because they have the same number of electrons.
Which of the following elements has the greatest attraction for electrons in a covalent bond?
Ge
As
Se
Br
Bi
All of the following properties of the alkaline earth metals increase going down the group except
atomic radius
first ionization energy
ionic radius
atomic mass
F, N, B
As you look down a group, ionization energy and electronegativity
increases
decreases
The amount of energy released when an electron is added to a neutral atom to form a negative ion
Atomic Radii
Ionization Energy
Electronegativity
Electron Afinity
Oxidation Number
Why do Group 18 elements have such high Ionization Energies?
They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.
They are non metals.
They are metals
Why do Group 1 elements have such low Ionization Energies?
They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.
They are non metals and therefore require more electrons to complete their outer energy level.
They are metals and its easier to give away the electrons in their outer energy level.
Why is there such an increase in 1st to 2nd Ionization energies for Lithium?
The 2nd ionization energy is higher because this energy level is full.
Lithium only has 1 electron in its outer energy level and therefore does not hold on to it very hard.
Why is the Electron Affinity in Group 1 elements so low?
They want to accept electrons
They have opposite charges which repel.
They do not want to accept electrons.
The Electron Affinity decreases from TOP TO BOTTOM in a GROUP.
TRUE
FALSE
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 a valence electron of magnesium is
+1
+2
+12
+24
Effective nuclear charge ________ across a period.
increases
decreases
stays the same
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.
Down the group , attraction between the nucleus and the valence electrons __________.
Increases due to shielding
Decreases due to shielding
Stays the same
What is the tendency of an atom to attract electrons towards itself in a bond?
atomic radius
ionization energy
shielding
Electronegativity
Why does ionization energy decrease going down a group?
Adding more energy levels places the valence e- further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Why does electronegativity increase across a period?
Adding more energy levels places the valence e- further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Which is smaller... Mg or Mg2+ ?
Mg because it gains an energy level
Mg due to extra electron repulsion
Mg2+ because of extra electron repulsion
Mg2+ because it loses electrons
List the following in order of smallest to largest ionization energy.
P, Cs, Co, Sr
P, Co, Sr, Cs
Cs, Sr, Co, P
Sr, Cs, Co, P
P, Co, Cs, Sr
P, Cs, Co, Sr
What happens to atomic radius across a period?
the atoms get bigger because the nucleus is bigger as more protons are added
the atoms get bigger because there are more valence electrons
the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus
Why doesn't having more protons increase the attraction down a column?
there are more valence electrons in the outermost energy level
actually, there aren't more protons in the nucleus down the column
as energy levels are added, non-valence electrons block the extra protons from attracting valence electrons
more neutrons block the extra protons
