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- 1. Multiple Choice
The trends on the periodic table are dependent on..
how attracted a valence electron is to the nucleus
how attracted valence electrons are to each other
how attracted a valence electrons is to a non valence electron
how attracted a non valence electron is to the nucleus
- 2. Multiple Choice
What makes a valence electron more attracted to the nucleus?
less distance between the nucleus and having less protons
less distance between the nucleus and having more protons
more distance between the nucleus and having less protons
more distance between the nucleus and having more protons
less distance and having more valence electrons
- 3. Multiple Choice
What is the tendency of an atom to attract electrons towards itself in a bond?
atomic radius
ionization energy
shielding
Electronegativity
- 4. Multiple Choice
The higher the ionization energy...
the more attracted the valence electron is to the nucleus so it is harder to remove
the less attracted the valence electron is to the nucleus so it is easier to remove
the more attracted the valence electron is to another electron, so it is harder to remove
the more repelled a valence electron is to another electron, so it is easier to remove
- 5. Multiple ChoiceWhich is larger... P or P3- ?P3- because it gains an energy levelP3- due to extra electron repulsionP because it loses an energy levelP because of extra electron repulsion
- 6. Multiple Choice
Why does ionization energy decrease going down a group?
Adding more energy levels makes the ve- further from the nucleus so it is easier to remove
There are more valence electrons in the outer shell so the ve- is easier to remove
There are more protons in the nucleus so the ve- is easier to remove
There are less protons in the nucleus so the ve- is easier to remove
- 7. Multiple ChoiceWhy does electronegativity increase across a period?Adding more energy levels makes the ve- further from the nucleusThere are more valence electrons in the outer shellThere are more protons in the nucleusThere are less protons in the nucleus
- 8. Multiple ChoiceWhich is smaller... Mg or Mg2+ ?Mg because it gains an energy levelMg due to extra electron repulsionMg2+ because of extra electron repulsionMg2+ because it loses an energy level
- 9. Multiple ChoiceList the following in order of weakest to strongest ionization energy.
P, Cs, Co, SrP, Co, Sr, CsCs, Sr, Co, PSr, Cs, Co, PP, Co, Cs, Sr - 10. Multiple ChoiceList the following from largest to smallest atomic radius.
P, Cs, Co, SrP, Co, Sr, CsP, Cs, Co, SrCs, Sr, Co, PSr, Cs, Co, P - 11. Multiple Choice
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 ve-
more neutrons block the extra protons
- 12. Multiple Choice
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 ve-
the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus
the atoms get bigger because there are more energy levels
- 13. Multiple Choice
Element Z has more protons than element Y, but both have 4 energy levels. Which statement is true?
Y is smaller and would attract electrons more in a bond
Y is bigger and would attract electrons more in a bond
Z is smaller and would attract electrons more in a bond
Z is bigger and would attract electrons more in a bond
- 14. Multiple Choice
Nitrogen is a _ so it will _ electrons when forming an ion.
metal, lose
metal, gain
nonmetal, lose
nonmetal, gain
- 15. Multiple Choice
Nitrogen will gain _ ve- to have a charge of _.
5 , -5
3, +3
3, -3
5, +5
- 16. Multiple Choice
A full valence shell is considered having _ ve-.
0
2
6
8
- 17. Multiple Choice
Which of the following lose all their ve- when forming an ion?
metals
nonmetals
metalloids
depends on how many ve- the element has
- 18. Multiple Choice
Which has a higher electronegativity.. Rb or Sr?
Rb, because with more p+ in its nucleus it attracts e- more
Sr, because with more p+ in its nucleus it attracts e- more
Rb, because with more nrg levels the ve- are closer to/ more attracted to the nucleus
Sr, because with more nrg levels the ve- are closer to/ more attracted to the nucleus
- 19. Multiple Choice
Which has a higher ionization energy.. N or As?
N, because with more p+ in its nucleus it attracts e- more making them harder to remove.
As, because with more p+ in its nucleus it attracts e- more making them harder to remove.
As, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.
N, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.
- 20. Multiple Choice
Look at the bohr models of Li and Be. Imagine the first valence electron was already removed from both atoms, and now you are going to remove the second valence electron. The energy required to remove the second valence electron is called second ionization energy. Would lithium or beryllium have a higher second ionization energy ?
Li, because it has more protons
Be, because it has more protons
Li, because the second valence electron comes from an energy level closer to the nucleus
Be, because the second valence electron comes from an energy level closer to the nucleus
Li, because the beryllium has two valence electrons that repel each other
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