Term
Which of the following atoms will have similar chemistry?
Na, Cu, K, N, Cs, |
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Definition
| Na, K, and Cs since they are in the same column of the periodic chart. |
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Term
How many valence electrons are in this electron configuration?
1s22s22p63s23p64s23d104p5 |
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Definition
Valence electrons exist in the orbital(s) at the highest energy level. The orbital(s) at the highest energy level have the largest number in front of them. In this case, 4s and 4p have the largest number in front, so there are seven valence electrons. |
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Term
A. Columns 1b-8b represent what kind of metals in the periodic chart?
B. In columns 1a-8a, what is the shortcut to know how many valence electrons are in an atom? |
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Definition
A. transistional metals
B. In columns 1a-8a, you can determine the number of valence electrons simply by looking to see what column the atom is in. For example, Na has 1 valence electron and we know this because Na is in the 1a column. |
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Term
| The noble gases are in column (a.)_____ and they are unique because they have the (b.)_____ number of valence electrons |
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Definition
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Term
What type of compound has a positive charge and why?
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Definition
| Ionic compounds have a positive charge because they give away electrons which are negatively charged. Thus, this creates a positive charged ion. |
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Term
| What is a covalent compound? |
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Definition
| It is a compound consisting only of nonmetals. Covalent compounds share electrons. |
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Term
a. What is ionization potential?
b. What is electronegativity? |
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Definition
a. The ionization potenial is the amount of energy needed in order to take an electron away from an atom.
b. Electronegativity is a mesure of how strongly an atom attracts extra electrons to itself. |
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Term
| Explain why the ozone is needed for earth. |
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Definition
| It makes life possible on earth by shielding the ultraviolet rays from the sun to the earth. |
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Term
What is the lewis structure for carbon?
What is the lewis structure for Cl?
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Definition
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Term
Write the chemical formulas for the following compounds:
a. aluminum oxide
b. chromium(III) chloride
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Definition
a. Al is in group 3A, so it wants a charge of 3+. Oxygen is in group 6A, so oxide will have a charge of 2-.
Ignoring the signs and switching the numbers gives us Al2O3.
b. Cr is an exception, because there is a Roman numeral in the name. The numeral tells us that Cr
want a charge of 3+. Chlorine is in group 7A, so chloride will have a charge of 1-. Ignoring the signs and switching the numbers gives us CrCl
3. |
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Term
Order the following atoms in terms of increasing ionization potential: Sr, Ra, Mg.
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Definition
Ionization potential decreases as you go down the chart. Thus, the order is Ra < Sr < Mg. |
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Term
Which atom has the greatest desire for extra electrons: Ge, Ca, or Br? |
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Definition
Electronegativity is a measure of an element’s desire for electrons. It increases as you move to the right on the chart, so Br has the greatest desire for electrons. |
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Term
Draw the Lewis structures for the following molecules:
a. NF3
b. CCl2S
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Definition
a. [image]
B. :Ċİ:
ı
:Ċİ- C -S:
● ● ●●
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Term
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Definition
| A charactertistic of atoms that varies regularly across the periodic chart |
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Term
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Definition
| A shared pair of valence electrons that holds atoms together in covalent compounds |
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