Question

element

protons

electrons

valence e

metal/nonmetal
for full valence shell
new # of electrons
new charge
ion that forms
sodium na
11
11
1
m
give 1
11 - 1 = 10
1+
na 1+
chlorine cl
magnesium mg
oxygen o
nitrogen n

Explanation:

To solve this, we use the properties of atoms (protons = electrons in neutral state, valence electrons, metal/nonmetal, electron gain/loss for octet, new electrons, charge, and ion formula). Let's fill each row:

Chlorine (Cl)

Step 1: # Protons

Atomic number of Cl is 17, so protons = 17.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 17.

Step 3: Valence Electrons

Cl is in group 17, so valence electrons = 7.

Step 4: Metal/Nonmetal

Cl is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. Cl needs \( 8 - 7 = 1 \) electron (gain 1).

Step 6: New # of Electrons

\( 17 + 1 = 18 \).

Step 7: Ionic Charge

Gaining 1 electron → charge = \( 1^- \).

Step 8: Ion Formula

\( \text{Cl}^- \).

Magnesium (Mg)

Step 1: # Protons

Atomic number of Mg is 12, so protons = 12.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 12.

Step 3: Valence Electrons

Mg is in group 2, so valence electrons = 2.

Step 4: Metal/Nonmetal

Mg is a metal (M).

Step 5: For Full Valence Shell

Metals lose electrons. Mg loses 2 electrons (give 2).

Step 6: New # of Electrons

\( 12 - 2 = 10 \).

Step 7: Ionic Charge

Losing 2 electrons → charge = \( 2^+ \).

Step 8: Ion Formula

\( \text{Mg}^{2+} \).

Oxygen (O)

Step 1: # Protons

Atomic number of O is 8, so protons = 8.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 8.

Step 3: Valence Electrons

O is in group 16, so valence electrons = 6.

Step 4: Metal/Nonmetal

O is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. O needs \( 8 - 6 = 2 \) electrons (gain 2).

Step 6: New # of Electrons

\( 8 + 2 = 10 \).

Step 7: Ionic Charge

Gaining 2 electrons → charge = \( 2^- \).

Step 8: Ion Formula

\( \text{O}^{2-} \).

Nitrogen (N)

Step 1: # Protons

Atomic number of N is 7, so protons = 7.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 7.

Step 3: Valence Electrons

N is in group 15, so valence electrons = 5.

Step 4: Metal/Nonmetal

N is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. N needs \( 8 - 5 = 3 \) electrons (gain 3).

Step 6: New # of Electrons

\( 7 + 3 = 10 \).

Step 7: Ionic Charge

Gaining 3 electrons → charge = \( 3^- \).

Step 8: Ion Formula

\( \text{N}^{3-} \).

Filled Table:

Element	# Protons	# Electrons	Valence e⁻	Metal/Nonmetal	For Full Valence Shell	New # of Electrons	Ionic Charge	Ion Formula
Chlorine (Cl)	17	17	7	N	gain 1	\( 17 + 1 = 18 \)	\( 1^- \)	\( \text{Cl}^- \)
Magnesium (Mg)	12	12	2	M	give 2	\( 12 - 2 = 10 \)	\( 2^+ \)	\( \text{Mg}^{2+} \)
Oxygen (O)	8	8	6	N	gain 2	\( 8 + 2 = 10 \)	\( 2^- \)	\( \text{O}^{2-} \)
Nitrogen (N)	7	7	5	N	gain 3	\( 7 + 3 = 10 \)	\( 3^- \)	\( \text{N}^{3-} \)

(Note: For "nitrogen N" in the table, the atomic symbol is actually \( \text{N} \), and the steps follow the same logic as above.)

Answer:

To solve this, we use the properties of atoms (protons = electrons in neutral state, valence electrons, metal/nonmetal, electron gain/loss for octet, new electrons, charge, and ion formula). Let's fill each row:

Chlorine (Cl)

Step 1: # Protons

Atomic number of Cl is 17, so protons = 17.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 17.

Step 3: Valence Electrons

Cl is in group 17, so valence electrons = 7.

Step 4: Metal/Nonmetal

Cl is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. Cl needs \( 8 - 7 = 1 \) electron (gain 1).

Step 6: New # of Electrons

\( 17 + 1 = 18 \).

Step 7: Ionic Charge

Gaining 1 electron → charge = \( 1^- \).

Step 8: Ion Formula

\( \text{Cl}^- \).

Magnesium (Mg)

Step 1: # Protons

Atomic number of Mg is 12, so protons = 12.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 12.

Step 3: Valence Electrons

Mg is in group 2, so valence electrons = 2.

Step 4: Metal/Nonmetal

Mg is a metal (M).

Step 5: For Full Valence Shell

Metals lose electrons. Mg loses 2 electrons (give 2).

Step 6: New # of Electrons

\( 12 - 2 = 10 \).

Step 7: Ionic Charge

Losing 2 electrons → charge = \( 2^+ \).

Step 8: Ion Formula

\( \text{Mg}^{2+} \).

Oxygen (O)

Step 1: # Protons

Atomic number of O is 8, so protons = 8.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 8.

Step 3: Valence Electrons

O is in group 16, so valence electrons = 6.

Step 4: Metal/Nonmetal

O is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. O needs \( 8 - 6 = 2 \) electrons (gain 2).

Step 6: New # of Electrons

\( 8 + 2 = 10 \).

Step 7: Ionic Charge

Gaining 2 electrons → charge = \( 2^- \).

Step 8: Ion Formula

\( \text{O}^{2-} \).

Nitrogen (N)

Step 1: # Protons

Atomic number of N is 7, so protons = 7.

Step 2: # Electrons (neutral)

Neutral atom: electrons = protons = 7.

Step 3: Valence Electrons

N is in group 15, so valence electrons = 5.

Step 4: Metal/Nonmetal

N is a nonmetal (N).

Step 5: For Full Valence Shell

Nonmetals gain electrons. N needs \( 8 - 5 = 3 \) electrons (gain 3).

Step 6: New # of Electrons

\( 7 + 3 = 10 \).

Step 7: Ionic Charge

Gaining 3 electrons → charge = \( 3^- \).

Step 8: Ion Formula

\( \text{N}^{3-} \).

Filled Table:

Element	# Protons	# Electrons	Valence e⁻	Metal/Nonmetal	For Full Valence Shell	New # of Electrons	Ionic Charge	Ion Formula
Chlorine (Cl)	17	17	7	N	gain 1	\( 17 + 1 = 18 \)	\( 1^- \)	\( \text{Cl}^- \)
Magnesium (Mg)	12	12	2	M	give 2	\( 12 - 2 = 10 \)	\( 2^+ \)	\( \text{Mg}^{2+} \)
Oxygen (O)	8	8	6	N	gain 2	\( 8 + 2 = 10 \)	\( 2^- \)	\( \text{O}^{2-} \)
Nitrogen (N)	7	7	5	N	gain 3	\( 7 + 3 = 10 \)	\( 3^- \)	\( \text{N}^{3-} \)

(Note: For "nitrogen N" in the table, the atomic symbol is actually \( \text{N} \), and the steps follow the same logic as above.)