Clicker Questions Nov 14/17, 2014 Unit 2 review:
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What are the “outermost” electrons in an atom or ion called?
a. Outliers
b. valiant electrons
c. valence electrons
d. orbiters.
How many valence electrons are in an atom of gallium?
a. 3
b. 13 c. 18 d. 31
How many valence electrons are in an atom of lead?
a. 54
b. 28 c. 4
d. 2
How many valence electrons are in an atom of bromine?
a. 7
b. 17 c. 18 d. 35
How many valence electrons are in an atom of neon?
a. 20.
B. 10 c. 8
d. 2
The number of valence electrons for a given atom that lies in a “tall” column may be identified
by numbering the 8 tall columns in order from left to right.
a. T
b. F
Since boron is in tall column #3….boron probably has 3 valence electrons; and, since carbon is in
tall column #4….carbon probably has 4 valence electrons.
a. T
b. F
The number of valence electrons for a given atom can also be identified by counting the “s” and
“p” electrons found in the abbreviated electron configuration on your periodic table
a. T
b. F
When “main block” atoms become stable by forming an ionic compound, they atoms (now
called ions) then have the same number of electrons as a noble gas atom.
a. T
b. F
When a sodium atom becomes a sodium ion, what noble gas will it be isoelectronic to?
a. He
b. Ne c. Ar d. Kr
When a beryllium atom becomes a beryllium ion, what noble gas will it be isoelectronic to?
a. He
b. Ne c. Ar d. Kr
When a fluiorine atom becomes a fluoride ion, what noble gas will it be isoelectronic to?
a. He
b. Ne c. Ar d. Kr
When a sulfur atom becomes a sulfide ion, what noble gas will it be isoelectronic to?
a. He
b. Ne c. Ar d. Kr
In the ionic compound, CaCl2, what noble gas are the ions isoelectonic to?
a. He
b. Ne c. Ar d. Kr
In the ionic compound, MgF2, what noble gas are the ions isoelectronic to?
a. He
b. Ne c. Ar d. Kr
When an atom gains electrons, it is called a cation.
a. T
b. F
When an atom gains protons, it is called a cation.
a. T
b. F
When an atom loses electrons, it is called a cation.
a. T
b. F
19. When an atom gains electrons, it is called an anion.
a. T
b. F
20. Cations are negatively charged ions.
a. T
b. F
21. Anions are negatively charged ions.
a. T
b. F
22. A symbol of an ion must include a charge written to its upper right.
a. T
b. F
23. A symbol of an ion must include a Roman numeral.
a. T
b. F
24. What is the electron configuration for an ion of Ca?
a. 1s2 2s2 2p6 3s2 3p 4s2
b. 1s2 2s2 2p6 3s2 3p6 4s4
c. 1s2 2s2 2p6 3s2 3p6 4s2 4p2
d. 1s2 2s2 2p6 3s2 3p6
25. What is the electron configuration for an anion of oxygen?
a. 1s2 2s2 2p4
b. 1s2 2s2 2p6
c. 1s2 2s2 2p5
d. 1s2 2s2 2p8
26. When a “main block” atom forms an ion, that ion’s electron configuration often ends in “s2p6”
a. T
b. F
27. Which of the following pairs of atoms is most likely to form an ionic compound?
a. He and Kr
b. Cs and Ba
c. Cd and I
d. F and Cl
28. Which of the following pairs of atoms is most likely to form an ionic compound?
a. Ti and Cl
b. Rb and Ag
c. Cl and Br
d. Pb and Ar
29. A binary ionic compound should contain 2 different metal ions.
a. T
b. F
30. A binary ionic compound should contain 2 different nonmetal ions
a. T
b. F
31. A binary ionic compound should contain 1 kind of metal ion and 1 kind of nonmetal ion.
a. T
b. F
32. The cation should be written first in an ionic compound.
a. T
b. F
33. Where is the “subscript” for an ion found in an ionic compound’s formula?
a. Below and to the right of the ion’s symbol
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b. Above and to the right of the ion’s symbol.
c. Below and to the left of the ion’s symbol.
d. Above and to the left of the ion’s symbol.
As you write a formula by doing a “drop and swap”, what should you remember to do?
a. Simplify the subscripts.
b. Omit the + and – signs.
c. Keep the polyatomic ion intact.
d. All of the above.
When you write the name for an ionic compound, you should
a. Change the ending of the polyatomic anions to –ide.
b. Change the ending of the monatomic (single atom) anions to –ide.
c. Change the ending of every anion to – ide.
d. Change the ending of the cation to –ide.
A Roman numeral is used
a. When naming every ionic compound.
b. When naming ionic compounds that have polyatomic ions.
c. When naming ionic compounds that have a cation with several common charges.
d. When naming ionic compounds that are identified as being acids.
Which of the following choices provides both a correct formula and name for the given acid.
a. HCl = hydrochlorous acid
b. HClO2 = hydrochloric acid
c. HClO3 = chloric acid
d. HCLO4 = chlorous acid
When naming an acid, it is important to notice whether the anion contains oxygen atoms.
a. T
b. F
When the anion of an acid contains oxygen atoms, you should include “hydro” as the prefix in
the acid’s name.
a. T
b. F
When the anion of an acid does not contain oxygen atoms, you should include “hydro” as the
prefix to the acid’s name.
a. T
b. F
In which of the following are both the symbols and names of the ions stated correctly.
a. Pb2+ is plumbic; Pb4+ is plumbous
b. Fe2+ is ferric; Fe3+ is ferrous
c. Sn2+ is stannic; Sn4+ is stannous
d. Cu2+ is cupric; Cu1+ is cuprous
As you move through a row of the periodic table from left to right, what happens to the energy
that is needed to remove an electron from the atoms (what happens to the ionization energy of
the atoms)?
a. It increases
b. It descreases
c. It stays the same
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d. It varies unpredictably
As you move through a row of the periodic table from left to right, what happens to the radius
of the atoms?
a. It increases.
b. It decrases.
c. It stays the same.
d. It varies unpredictably.
Ionic compounds are composed of metallic elements (cations) and nonmetallic elements
(anions)?
a. T
b. F
Ionic compounds are neutral.
a. T
b.F
Ionic compounds have low melting points (melt at low temperatures).
a. T
b. F
Ionic compounds conduct electricity when melted or dissolved in water.
a. T
b. F
Ionic compounds conduct electricity when in the solid state.
a. T
b. F
Ionic compounds are usually found in either the gaseous or in the liquid state.
a. T
b. F
Ionic compounds are usually found in the solid state.
a. T
b. F
10 points…Open ended question (not a multiple choice question):
Similar to this: Write a formula for barium hydroxide; then, explain in detail what your “steps”
were or how you know your formula is correct.
Example incorrect answers:
BaOH because I put the cation first and the anion second.
BaOH2 because I put the cation first and the anion second and do a drop swap.
Example correct answers:
Ba(OH)2 is the correct formula because after writing the symbol of the cation
first and the symbol for the anion second, I put parentheses around the polyatomic ion (which is the
hydroxide ion). Then, I “dropped and swapped the two charges”, removed the “+” and “–“signs, and
checked to make sure that I didn’t need to simplify my two subscripts. Last, I am sure that this is the
correct formula because I have checked that the ions combined give me a neutral formula:
1 (Ba) + 2 (OH) = 0
1 (+2) + 2 (-1) = 0.
52. 5 points open ended question (NOT multiple choice).
Similar to this: Name the following compounds. Explain how you chose your Roman numerals:
CuO and Cu2O.
Example incorrect answers:
Their names are copper oxide because Cu is copper and O is oxide.
Their names are copper(I) oxide and copper (II) oxide because the first formula has a 1
and the second formula has a 2.
Example correct answer:
I call CuO copper(II) oxide because the compound’s formula is neutral. This means that
the one “Cu” + the one “Oxy” charges’ must add up to zero: Cu + Oxy = zero. Since I know
that the Oxy is always “-2”, then the Cu must be +2. 1 (x) + 1 (-2) = 0 x = +2
I call Cu2O copper(I) oxide because the compound’s formula is neutral. This means that
the two “Cu” and the one “oxy” charges’ must add up to zero: 2 Cu + 1 Oxy = zero. Since I
know that the Oxy is always “-2”, then the Cu must be +1. 2 (x) + 1 (-2) = 0 x = +1
53. Open ended: 15 questions, 2 points each.
“Name the following ionic compounds”. You will be given 15 formulas.
Examples similar in difficulty:
Given NH4Cl
Incorrect answer: ammonium chlorine
Correct answer: ammonium chloride
Given FePO4
Incorrect answer: iron phosphate
Incorrect answer: iron(4) phosphate
Incorrect answer: iron(IV) phosphate
Correct answer: iron(III) phosphate
How did I get it?
1 Fe + 1 (PO4) = 0
1 x + 1 (-3) = 0
so, x = +3
And this means: iron(III)