Answer these QUIZ REVIEW questions – everybody in your group needs to understand the answers, and I will feel free to call on anybody using the popsicle sticks:
1.
Which group is oxygen in? VIA
2.
Which period is chlorine in? 3
3.
When you write the name of an element, should it be capitalized? No
4.
How many protons does P have? 15
5.
How many neutrons would you expect uranium, element #92 to have? 146
6.
An element lost 2 electrons from what it had when it was neutral, what should its charge now be? +2
7.
What is the mass number of Be, and what does it tell you about Be? 9, which tells you that there are a
total of 9 protons + neutrons (which equals the mass number)
8.
Which element is in period 3, group 7A (VIIA)? Chlorine
9.
When drawing Bohr models, how many energy levels would the element in question 8 have? 3
10.
How many valence electrons should you plan to draw on every element in group VA? 5
11.
How many protons, neutrons, and electrons does Kr have? 36 protons, 48 neutrons, 36 electrons (if
neutral)
12.
Why aren’t things in group 8A (VIIIA) reactive under ordinary circumstances? Because they have a full outer energy level already. Don’t need to change anything about their valence electrons, so don’t
need to bond.
13.
Why do the ions in an ionic bond “stick together”? Because they have opposite charges, and
oppositely charged ions attract each other in ionic bonds.
14.
What is/are the difference(s) between ionic and covalent bonds? Both types of bonds are generally done to make it so that the atoms’ outer energy levels are full, and/or have additional stability. In an ionic bond, the atoms give or take electrons, which gives the atoms + or – charges, so we call them ions. The ions are attracted to each other because of the opposite charges that they have obtained.
In covalent bonds, the atoms share electrons so that they can all pretend to have enough for a full
outer energy level. They have to share equally, like in kindergarten.
15.
What do elements in groups IA and IIA generally make when they bond to elements in group VIA or
VIIA? Salts, with ionic bonds.
16.
How many calcium and fluorine ions would you expect to bond to each other? For this ionic bond to add up to zero, you need 1 Ca atom (+2) and 2 F atoms (-1, -1)

17.
Which element is in group 5A and period 4? Arsenic
18.
How many Na and O ions would you expect to bond to each other? What’s the formula? 2 Na atoms that are each -1 in charge, 1 O atom that is -2 in charge. Adds up to zero. Formula is Na
2
O
19.
Draw the previous substance using Lewis Dot Diagrams.
The drawing below is pretty good, but I’d have you circle the charges when you were done.
+1
+1 x x
-2
20.
What is the mass of a proton? Where is it located in an atom? 1 amu, nucleus
21.
What is the mass of a neutron? Where is it located in an atom? 1 amu, nucleus
22.
What is the mass of an electron? Where is it located in an atom? 1/1836 amu, electron cloud around
nucleus
23.
What do we call the diagrams with rings around the nucleus? Bohr Models
THIS WAS ALSO ON THE PLAN:
Share your Lewis Dot Diagram drawings you made last week for H2O and the two ionic compounds written on the board (LiF, MgF).
Discuss how to draw CO2.
Extra Questions I just thought of and that you should be able to answer (part of classwork on Friday):
A.
What are valence electrons?
B.
When 2 elements bond in an ionic bond, what should the charges add up to?
C.
What are oxidation numbers, and what are they useful for?
D.
What does cohesion have to do with water droplets?
E.
Where are the metals on the periodic table?
F.
Where are the nonmetals on the periodic table?
G.
Where are the metalloids on the periodic table?
H.
What type of bond is typically formed between a metal and a nonmetal?
I.
What type of bond is typically formed between nonmetals and nonmetals?
J.
What sort of bonds typically form between two metals?
K.
Draw the bond between any atom in group IIA and any atom in group VIIA.