Question

magnesium oxygen magnesium oxide electrons? lost or gained? charge of magnesium lon charge of oxygen lon x. stop and think element with electron configuration # protons # electrons # valence electrons metal or nonmetal to get a full outer shell new # of electrons new charge lon that forms ex: sodium (na) 2,8,1 11 11 1 m lose 1 11 - 1 = 10 1+ na +1 ex: chlorine (cl) 2,8,7 17 17 7 nm gain 1 17 + 1 = 18 -1 cl - 1 magnesium (mg) 2,8,2 oxygen (o) 2,6 nitrogen (n) 2,5 xi. trend for lonic charge - if these charges are not on the top of your periodic table, add them now. xii. common lons formed: charges listed on slide periodic table of the elements xiii. covalent bonding a. electrons are _ between _ elements. b. covalent bonds are also called _ bonds as they form molecules.

Explanation:

Step1: Analyze Magnesium (Mg)

Magnesium has an electron configuration of \(2, 8, 2\). The number of protons is equal to the atomic number, so for Mg, protons \(= 12\). Electrons are also \(12\) (neutral atom). Valence electrons are \(2\). Mg is a metal (M). To get a full outer shell, it loses 2 electrons. New electrons: \(12 - 2 = 10\). Charge: \(2+\) (since it loses 2 electrons, positive charge). Ion formed: \(Mg^{2+}\).

Step2: Analyze Oxygen (O)

Oxygen has an electron configuration of \(2, 6\). Protons \(= 8\) (atomic number 8), electrons \(= 8\) (neutral). Valence electrons \(= 6\). O is a non - metal (NM). To get a full outer shell, it gains 2 electrons. New electrons: \(8 + 2 = 10\). Charge: \(-2\) (gains 2 electrons, negative charge). Ion formed: \(O^{2-}\).

Step3: Analyze Nitrogen (N)

Nitrogen has an electron configuration of \(2, 5\). Protons \(= 7\) (atomic number 7), electrons \(= 7\) (neutral). Valence electrons \(= 5\). N is a non - metal (NM). To get a full outer shell, it gains 3 electrons. New electrons: \(7+3 = 10\). Charge: \(-3\) (gains 3 electrons, negative charge). Ion formed: \(N^{3-}\).

Step4: Covalent Bonding (Part XIII)

Part A

In covalent bonding, electrons are shared between non - metal elements. This is because non - metals have relatively high electronegativities and tend to share electrons rather than transfer them (as in ionic bonding).

Part B

Covalent bonds are also called molecular bonds as they form molecules. Molecules are the basic units of covalent compounds, unlike ionic compounds which form lattices of ions.

Answer:

For the table (Stop and Think section):

• Magnesium (Mg):
• # protons: \(12\)
• # electrons: \(12\)
• # valence electrons: \(2\)
• Metal or non - metal: \(M\)
• To get a full outer shell: Lose \(2\)
• New # of electrons: \(10\)
• New Charge: \(2+\)
• Ion that forms: \(Mg^{2+}\)
• Oxygen (O):
• # protons: \(8\)
• # electrons: \(8\)
• # valence electrons: \(6\)
• Metal or non - metal: \(NM\)
• To get a full outer shell: Gain \(2\)
• New # of electrons: \(10\)
• New Charge: \(-2\)
• Ion that forms: \(O^{2-}\)
• Nitrogen (N):
• # protons: \(7\)
• # electrons: \(7\)
• # valence electrons: \(5\)
• Metal or non - metal: \(NM\)
• To get a full outer shell: Gain \(3\)
• New # of electrons: \(10\)
• New Charge: \(-3\)
• Ion that forms: \(N^{3-}\)

For Part XIII (Covalent Bonding):

• Part A: Electrons are \(\boldsymbol{shared}\) between \(\boldsymbol{non - metal}\) elements.
• Part B: Covalent bonds are also called \(\boldsymbol{molecular}\) bonds as they form molecules.