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Bonding Practice and other Chapter 8 Test Practice Homework
1. Which has a higher ionization potential, carbon or oxygen? Why?
2. Which has a greater atomic radius, cobalt or iridium? Why?
3. Which has a greater atomic mass, strontium or magnesium? Why?
4. Which has a greater electronegativity, nitrogen or phosphorous? Why?
5. Which has a greater ionization potential, aluminum or gallium? Why?
6. Which has a greater electronegativity, gold or platinum? Why?
7. Which has a greater atomic radius, calcium or germanium? Why?
8. Draw the Lewis Dot Structures and bonding for a molecule made up of H and O atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
9. Draw the Lewis Dot Structures and bonding for a molecule made up of Sr and S atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
10. Draw the Lewis Dot Structures and bonding for a molecule made up of C and O atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
11. Draw the Lewis Dot Structures and bonding for a molecule made up of Sn (II) and N atoms. If there
are multiple options for the bonding structure, you may choose any valid setup. If there is only one
possible option, write the chemical formula and identify any charged particles.
12. Draw the Lewis Dot Structures and bonding for a molecule made up of Be and C atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
13. Draw the Lewis Dot Structures and bonding for calcium phosphide, including indication of any
cations and anions.
14. Draw the Lewis Dot Structures and bonding for hexane (C6H14), including indication of any cations
and anions.
15. Draw the Lewis Dot Structures and bonding for diatomic oxygen, including indication of any cations
and anions.
16. Draw the Lewis Dot Structures and bonding for Copper (IV) Oxide, including indication of any cations
and anions.
17. Draw the Lewis Dot Structures and bonding for H2CO2, including indication of any cations and
anions.
18. Draw the complete Lewis Dot Structures and bondings for ozone, including indication of any cations
and anions.
19. Write the complete electron configuration for Osmium.
20. Write the abbreviated electron configuration for Phosphorus
21. Write the abbreviated electron configuration for yttrium
22. Draw the Lewis Dot Structures and bonding for pentanol, including indication of any cations and
anions.
23. Draw the Lewis Dot Structures and bonding for Zn (IV) Nitride, including indication of any cations
and anions.
24. Which has a higher ionization potential, boron or aluminum? Why?
25. Which has a greater atomic radius, magnesium or sulfur? Why?
26. Which has a greater electronegativity, iodine or xenon? Why?
27. Which has a greater electronegativity, lithium or oxygen? Why?
28. Which compound would take the most energy to break one of its bonds, LiF, CO2, N3, or H2O?
29. Write the abbreviated electron configuration for vanadium.
30. Write the full electron configuration for lawrencium.
Answers
1. Which has a higher ionization potential, carbon or oxygen? Why?
Ionization potential is the amount of energy it would require to take off an electron from the atom. As
you go towards the right, there is less and less interest in losing an electron, since they are so close to
being full. So oxygen will require more energy, and thus have a higher ionization potential.
2. Which has a greater atomic radius, cobalt or iridium? Why?
As you add more energy levels, the electrons are further away. Therefore iridium would have a larger
radius, since it has electrons at energy level 6, while cobalt only has them at energy level 4.
3. Which has a greater atomic mass, strontium or magnesium? Why?
Strontium. The trend is that as you go down the periodic table, there are more protons, neutrons, and
electrons, and thus more mass.
4. Which has a greater electronegativity, nitrogen or phosphorous? Why?
Electronegativity is how strongly an atom will pull in ADDITIONAL electrons. As you go down,
electronegativity decreases because the nucleus’ pull is further away (or more shielded by other
electrons). That means nitrogen will have the greater electronegativity.
5. Which has a greater ionization potential, aluminum or gallium? Why?
Aluminum. As in the question before, the nucleus’ pull is greater at lower energy levels. So it will take
more energy to pull off the nearby electrons in aluminum, than the more distant ones in gallium.
6. Which has a greater electronegativity, gold or platinum? Why?
Gold, because it is closer to the right, it will be more interested in pulling in more electrons to fill up to
being a noble gas.
7. Which has a greater atomic radius, calcium or germanium? Why?
Calcium. Remember the radius decreases as you go towards the right because you increase the number
of central protons without adding new energy levels, so the electrons are all pulled in a little tighter due
to all those protons in the middle.
8. Draw the Lewis Dot Structures and bonding for a molecule made up of H and O atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
O and H will make a covalent compound. Thus there are multiple options, the two most basic of which
are H2O or H2O2 (OH- is also even an option, where it gains an extra electron). There are not ions to
worry about. Here are their dot structures.
9. Draw the Lewis Dot Structures and bonding for a molecule made up of Sr and S atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
Because it is ionic, there will only be one combination. Here is the bonding:
And thus the compound formula is SrS, with ions of Sr2+ and S2-.
10. Draw the Lewis Dot Structures and bonding for a molecule made up of C and O atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
It is covalent, so there are options, but the most basic one is CO2. CO is doable, but the carbon gives the
oxygen one of its electrons, making the structure fairly difficult to ascertain. You could also probably
make an extended chain of carbon in the middle or oxygen on the edge, but why go to such trouble.
Whatever you come up with, make sure each atom has 8 electrons. Note that I moved the two shared
pairs next to each other to aid readability, but whatever way you draw it should be fine so long as two
pairings are shown.
11. Draw the Lewis Dot Structures and bonding for a molecule made up of Sn (II) and N atoms. If there
are multiple options for the bonding structure, you may choose any valid setup. If there is only one
possible option, write the chemical formula and identify any charged particles.
Sn (III) just means that the tin is each giving up 3 electrons. Nitrogen has 5 so needs 3. It is ionic due to
the metal tin, so a simple 1 to 1 ratio, it works out to!
The ions are Sn3+ and N3– and the formula is just SnN (you can include the III if you wish).
12. Draw the Lewis Dot Structures and bonding for a molecule made up of Be and C atoms. If there are
multiple options for the bonding structure, you may choose any valid setup. If there is only one possible
option, write the chemical formula and identify any charged particles.
Ionic given that Be is a metal, so just one possible combination…
Each Be gives up 2, each C gains 4, so the formula is Be2C and the ions are Be2+ and C4-.
13. Draw the Lewis Dot Structures and bonding for calcium phosphide, including indication of any
cations and anions.
Since calcium gives up 2 and phosphorus gains 3, they’ll combine until there are 6 gained and lost as…
The formula would thus be Ca3P2, the cation is Ca2+ and the anion is P3-.
14. Draw the Lewis Dot Structures and bonding for hexane (C6H14), including indication of any cations
and anions.
Covalent, and carbon needs the most so they are in the center. Single bond them, then start
surrounding them with hydrogen until you run out. You’d do any double bonds at this point, but no
need, they’re all already full!!!
However, there are actually some other isomers, as well that you could have done (and rotated
variations of these). But I’m happiest with the one above!
15. Draw the Lewis Dot Structures and bonding for diatomic oxygen, including indication of any cations
and anions.
Put them next to each other and share until full. Pretty simple hopefully. All the diatomics just share
this same way, it’s just a question of whether it’s a single, double, or triple bond.
16. Draw the Lewis Dot Structures and bonding for Copper (IV) Oxide, including indication of any cations
and anions.
Copper loses 4, oxygen gains 2. Therefore you end up with a structure of:
Each Copper lost 4, each oxygen gained 2, so Cu4+ is the cation, O2- is the anion, and the formula is CuO2.
17. Draw the Lewis Dot Structures and bonding for H2CO2, including indication of any cations and
anions.
Start with the C in the middle, then a couple Os around it. If you put the other two Hs around the
carbon, you’d end up not completing oxygen, so hold off on them and see where you need to go. You
end up double bonding one oxygen, and the hydrogen go around the C and the other O. If you got a
different answer, check that all atoms have 8 electrons, and you didn’t create electrons, then let me
know. Remember, we’re not going to be having weird circular connections (though they sometimes can
happen).
18. Draw the complete Lewis Dot Structures and bondings for ozone, including indication of any cations
and anions.
As a straight bonding exercise, you won’t be able to make ozone work, as we talked about in class. The
central atom can be full, but the edge atoms won’t have enough. Remember what happens is that the
central atoms gives one of its electrons away to a neighbor, then makes a double with the other atom.
Then the electron and double\single bond vacillate back and forth between the outside oxygens. There
are also charges where an atom has gained an electron, and a positive charge for the center atom.
Remember from the reading for extra credit, the single bond is more easily broken by ultraviolet
radiation, using it up and preventing it from reaching the Earth. I colorcoded the molecule below so you
can see the red electron being given back and forth to the two other oxygens in the diagrams (both of
which are needed).
19. Write the complete electron configuration for Osmium.
1s22s22p63s23p64s23d104p65s24d105p66s24f145d6
20. Write the abbreviated electron configuration for Phosphorus
Remember, you start with the noble gas the line before the element you are interested in, then finish…
[Ne]3s23p3
21. Write the abbreviated electron configuration for yttrium
[Kr]5s24d1
22. Draw the Lewis Dot Structures and bonding for pentanol, including indication of any cations and
anions.
So, the key question is were you able to remember the molecular formula yourself??? Alkanes are
usually prefixed by a number indicating their carbons. Pent = 5. So if it were pentane, it’d be C5H12
(surround all the carbons with hydrogens, which requires for the center ones, three for the ending
ones… in alkanes, H is always 2xC +2). But then it’s an alcohol. How do we turn an alkane into an
alcohol? Replace one H with OH.
Do I expect you to be able to determine the formulas for alkanes\alcohols from just the name? No.
Expect it for extra credit? Yes.
23. Draw the Lewis Dot Structures and bonding for Zn (IV) Nitride, including indication of any cations
and anions.
A longer chain!
That makes the formula Zn3N4, the anion N3- and the cation Zn4+.
24. Which has a higher ionization potential, boron or aluminum? Why?
Boron. Since it is higher up the same row, it will be harder to remove its electrons since the electrons
are held better by the nucleus.
25. Which has a greater atomic radius, magnesium or sulfur? Why?
Magnesium. Because as you go to the right in the same row, the radius decreases because there are
more protons at the center pulling all the electrons in a little closer.
26. Which has a greater electronegativity, iodine or xenon? Why?
Well, it’s tricky, because the usual trend for electronegativity is that atoms to the right want electrons
more. But that runs afoul when you hit the Noble Gases. Most of them will not take electrons at all.
This one actually does in a couple situations, but the electronegativity of iodine is greater, and that is the
trend you should be mindful of. Column 7A, not 8A, has the peak electronegativities.
27. Which has a greater electronegativity, lithium or oxygen? Why?
A more normal question. Oxygen. It is closer to being full, so will pull electrons more.
28. Which compound would take the most energy to break one of its bonds, LiF, CO2, N2, or H2O?
So, first we need to determine what types of bonds make each of these up. Lithium fluoride is ionic.
Carbon dioxide is double bonds (see problem 10). Diatomic nitrogen, if you draw it out, is a triple bond,
because each nitrogen needs 3 more electrons, and must get them by sharing. Water is two single
bonds. Which is hardest to break? Well which situation would be hardest to get someone to move
away in? A triple share is the hardest to split apart, it would take a lot of sorting out before they could
move free. Double bonds are next strongest, then single, and finally ionic (though as a whole, ionic
compounds are tough to break up due to their networked attraction between molecules, each specific
ion can move rather freely to other charged compounds.
30. Write the abbreviated electron configuration for vanadium.
[Ar]4s23d3
31. Write the full electron configuration for lawrencium.
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d1
Yes, don’t forget the extra 1 at the end on the right because it’s the hollowed out hole where the f row
comes out! There’s 15 elements in the f row, 14 for the f buildup, and 1 for the d that would be back in
that slot on the main table.