GT CHEMISTRY
Unit: Atomic Theory
Name: __________________________________________ Date: _______ MOD: _________
Atoms vs. Ions
Use the chart below the answer the following questions:
Atom
H
He
Li
Be
B
N
O
F
Ne
Na
Mg
Al
P
S
Cl
Ar
No.
Electrons
1
2
3
4
5
7
8
9
10
11
12
13
15
16
17
18
Subshell Electron
Configuration
1s1
1s2
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
1s2 2s2 2p6 3s1
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p6 3s2 3p3
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6
Ion
H-
No.
Electrons
1+1=2
Subshell Electron
Configuration
1s2
Li+
Be2+
B3+
N3O2F-
3-1=2
4-2=2
5-3=2
7 + 3 = 10
8 + 2 = 10
9 + 1 = 10
1s2
1s2
1s2
2
1s 2s2 2p6
1s2 2s2 2p6
1s2 2s2 2p6
Na+
Mg2+
Al3+
P3S2Cl-
11 - 1 = 10
12 - 2 = 10
13 - 3 = 10
15 + 3 = 18
16 + 2 = 18
17 + 1 = 18
1s2 2s2 2p6
1s2 2s2 2p6
1s2 2s2 2p6
2
1s 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6
1. Organize the atoms into three groups based on the common ion they form.
2. Examine the electron configurations of the ions formed for hydrogen, and
lithium-boron. These atoms lost electrons to obtain an electron configuration like
which element? __________________________________
GT CHEMISTRY
Unit: Atomic Theory
3. Examine the electron configurations of the ions formed for nitrogen to fluorine.
These atoms gained electrons to obtain an electron configuration like which
element? __________________________________
4. Examine the electron configurations of sodium to chlorine. These ions all have
electron configurations that end in what two things (a letter and number)?
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5. Why would atoms form ions? _____________________________________________
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6. Why are there no ions listed for Helium, Neon, and Argon? ___________________
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