completion________
_______corrections
Name: _________________________________________________________
Block: _____
Date: ______________
Problem Set #4 (U1, L17-24)
Vocab/Concepts: Fill in the blanks or circle the correct response in brackets.
1. In our model of the atom, electrons are arranged into ____________________, which are also known as energy
levels.
2. Energy levels that are _____________________ to the nucleus are lower in energy.
3. Electrons tend to go in to the ______________________________ energy shells first, until they are filled.
4. During a flame test, electrons jump from one energy level to another, causing _________________________ to be
given off.
5. The outermost shell in an atom is called the _________________________ shell, and electrons in that shell
are called ___________________________ electrons.
6. The outermost electrons are most important because __________________________________________________
______________________________________________________________________________________________.
7.
When there are more protons in the nucleus, the outermost electron’s attraction to the nucleus is [weaker]
[stronger].
8. When electrons are in higher energy levels, their attraction to the nucleus is [weaker] [stronger].
9. Elements toward the bottom left corner of the periodic table are called ___________________ and have a relatively
[strong] [weak] hold on their outermost electrons.
10. Elements toward the top right corner of the periodic table are called ___________________ and have a relatively
[strong] [weak] hold on their outermost electrons.
11. _______________________________ is a measure of how strongly an atom attracts electrons in chemical bonds.
12. When atoms of metals and nonmetals get together, the ______________________ atoms steal electrons from the
________________________ atoms. They then stick together. This is known as ____________________ bonding.
13. When an atom has a charge, it is called a(n) ___________.
14. When an atom gains one or more electrons, it becomes a(n) _________________________.
15. When an atom loses one or more electrons, it becomes a(n) _________________________.
16. In an ionic compound, the total charge must equal _______________________.
17. A group of nonmetal atoms that is bonded together to make a single charged particle is called a
_________________________________.
18. When forming ions, atoms tend to end up with _____________ valence electrons. This is known as the __________
rule.
19. (Extension - optional) Electron shells can be further divided into ____________________________, which are
labeled s, p, d, or f.
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Questions/Problems:
20. For each of the elements listed below, give
(a) The number of valence electrons.
(b) Instructions for it to form an ion that follows the octet rule (e.g. “gain two electrons”).
(c) The symbol for the ion it will form.
The first one has been completed as an example.
Element
(a)
Sr
2
(b)
(c)
Lose 2 electrons
Sr2+
Na
O
Br
N
Ga
Mg
21. For each pair of elements,
a) Draw Lewis dot representations of each element. Show the transfer of electrons that will occur when these elements
react. Use enough atoms of each element to make sure that each atom has a “full octet” (see example below).
b) Give the formula for the compound they will form together.
Al and O
a)
Al
O
b) Al2O3
Ba and Se
Al
O
O
Al3+ Al3+
O2- O2- O2-
Note: Al3+ (1s22s22p6) actually has 8 valence electrons in energy level 2, but they are not shown.
completion________
Na and S
Rb and F
Ga and Cl
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Sr and N
22.
23. Each entry in the chart below represents an ionic compound. The cation (positive ion), anion (negative ion),
chemical formula, and name are all listed. Fill in all the missing information in each entry. The first one is already
complete as an example.
Cation Anion
Fe2+
Cl–
Na+
Br−
Al3+
SO42−
Ca2+
O2−
Formula
Name
FeCl2
iron (II) chloride
AlBr3
GaAs
Li3P
rubidium telluride
aluminum oxide
magnesium nitride
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Cation Anion
K+
CO32−
Ba2+
NO3−
Al3+
PO43−
NH4+
SO42−
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Formula
Name
NaH2PO4
CaSO4
Na2SiO3
SrCrO4
rubidium nitrate
indium carbonate
sodium cyanide
magnesium hydroxide
strontium hydrogencarbonate
lithium perchlorate
The remainder of the problem set is an optional extension.
Read U1, Lessons 23 and 24 from the book. Then answer the questions that follow.
24. Why must a Roman numeral be used to indicate the charge on a transition metal ion?
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Remember, these are optional extension questions.
25. Fill in the chart below.
Cation Anion
Hg2+
Formula
Name
S2−
NiCl2
CuCO3
cobalt (II) sulfate
chromium (VI) oxide
26. Write the electron configuration for each of the following elements. You may use the noble gas abbreviation if you
wish.
(a) oxygen: _____________________________________________________________________________________
(b) chlorine: ____________________________________________________________________________________
(c) silver: ______________________________________________________________________________________
27. Draw a subshell model for vanadium (V), putting all the electrons in their appropriate places.