Question

b. turn on show formula. what is the formula of this compound? li2o
c. turn on show charge. what is the charge of each ion? li + li + o 2 - jnri

1. practice: use the gizmo to create stable compounds from the combinations given below. after transferring electrons, arrange the atoms to demonstrate the attraction between positively charged ions and negatively charged ions. click check to check each compound.

for each compound, click the camera ( ) icon to take a snapshot. right - click the image, and click copy image. paste each image into a blank document to turn in with this worksheet. write the ionic charges (such as ca²⁺) and chemical formulas below.
a. lithium and fluorine: li f
b. beryllium and oxygen: be o
c. magnesium and fluorine: mg f
d. aluminum and chlorine: al cl
e. beryllium and nitrogen be n

Explanation:

• Lithium (Li) and fluorine (F):
• Lithium is in Group 1 of the periodic table. Elements in Group 1 have 1 valence electron and tend to lose it to form a \(+1\) ion (\(Li^{+}\)).
• Fluorine is in Group 17. Elements in Group 17 have 7 valence electrons and tend to gain 1 electron to form a \(- 1\) ion (\(F^{-}\)).
• To form a neutral compound, the charges must balance. So, the chemical formula is \(LiF\) (1 \(Li^{+}\) and 1 \(F^{-}\)).
• Beryllium (Be) and oxygen (O):
• Beryllium is in Group 2. Elements in Group 2 have 2 valence electrons and tend to lose them to form a \(+2\) ion (\(Be^{2+}\)).
• Oxygen is in Group 16. Elements in Group 16 have 6 valence electrons and tend to gain 2 electrons to form a \(-2\) ion (\(O^{2 -}\)).
• The charges balance 1:1, so the chemical formula is \(BeO\).
• Magnesium (Mg) and fluorine (F):
• Magnesium is in Group 2. It forms a \(+2\) ion (\(Mg^{2+}\)).
• Fluorine forms a \(-1\) ion (\(F^{-}\)).
• To balance the charges (\(+2\) from \(Mg\) and \(-1\) from \(F\)), we need 2 \(F^{-}\) ions for every 1 \(Mg^{2+}\) ion. So the formula is \(MgF_{2}\).
• Aluminum (Al) and chlorine (Cl):
• Aluminum is in Group 13. It has 3 valence electrons and tends to lose them to form a \(+3\) ion (\(Al^{3+}\)).
• Chlorine is in Group 17. It forms a \(-1\) ion (\(Cl^{-}\)).
• To balance the \(+3\) charge of \(Al\) with \(-1\) charges of \(Cl\), we need 3 \(Cl^{-}\) ions. So the formula is \(AlCl_{3}\).
• Beryllium (Be) and nitrogen (N):
• Beryllium forms a \(+2\) ion (\(Be^{2+}\)).
• Nitrogen is in Group 15. It has 5 valence electrons and tends to gain 3 electrons to form a \(-3\) ion (\(N^{3 -}\)).
• To balance the charges, we use the least - common multiple of 2 and 3 (which is 6). For \(Be^{2+}\), we need 3 ions (\(3\times(+ 2)=+6\)) and for \(N^{3 -}\), we need 2 ions (\(2\times(-3)=-6\)). So the formula is \(Be_{3}N_{2}\).

Answer:

• A. Lithium and fluorine:
• Ionic charges: \(Li^{+}\), \(F^{-}\)
• Chemical formula: \(LiF\)
• B. Beryllium and oxygen:
• Ionic charges: \(Be^{2+}\), \(O^{2 -}\)
• Chemical formula: \(BeO\)
• C. Magnesium and fluorine:
• Ionic charges: \(Mg^{2+}\), \(F^{-}\)
• Chemical formula: \(MgF_{2}\)
• D. Aluminum and chlorine:
• Ionic charges: \(Al^{3+}\), \(Cl^{-}\)
• Chemical formula: \(AlCl_{3}\)
• E. Beryllium and nitrogen:
• Ionic charges: \(Be^{2+}\), \(N^{3 -}\)
• Chemical formula: \(Be_{3}N_{2}\)