1)Which of the following compounds has the largest lattice energy:

LiF
LiCl
NaF
NaCl

2)Which of the following compounds has the most ionic character in its bonding:
CaBr2
GeBr4
KBr
GaBr3

3)Using the electronegativity table on page 364 of your text, which end of the B-N bond is negative?
B
N
neither
both

4)The O-H bond in a water molecule is:
nonpolar covalent
ionic
polar covalent
ionic covalent

My answers are:
1)LiF
2)KBr
3)N
4)polar covalent

I just want to be completely sure of these answers before submitting them, since I just get one opportunity to do so. If someone could check this, it would be deeply appreciated. Also, if something is wrong, please explain... Thanks

#1 is a little confusing with the use of the word largest. I think it is common practice to list LiF as the largest lattice energy but technically it is the smallest number.

Lattice energies are as follows:
LiF = -1036 kJ/mol
NaF = -923 kJ/mol
LiCl = -853 kJ/mol
NaCl = -787 kJ/mol
Therefore, I think you answer to #1 is ok but do keep the negative in mind.

2, 3, and 4 look ok to me.

GeBr4

Your answers are mostly correct! Here's a review of each question:

1) Which of the following compounds has the largest lattice energy:
- Correct answer: LiF
- Lattice energy is the energy released when ions come together to form a solid crystal lattice. It depends on the magnitude of the charges and the sizes of the ions. Since LiF has the highest charges (Li+ and F-) and the smallest ions, it has the largest lattice energy.

2) Which of the following compounds has the most ionic character in its bonding:
- Correct answer: CaBr2
- Ionic character in a bond refers to the unequal sharing of electrons, where one atom has a greater control over the shared electrons. In general, metal cations and nonmetal anions tend to form more ionic bonds. Therefore, CaBr2, which consists of a metal (Ca) and a nonmetal (Br), has the most ionic character.

3) Using the electronegativity table on page 364 of your text, which end of the B-N bond is negative:
- Correct answer: N
- Electronegativity is a measure of an atom's ability to attract electrons in a bond. By comparing the electronegativity values for B (2.0) and N (3.0), we can see that N is more electronegative. Hence, N is the more negative end of the B-N bond.

4) The O-H bond in a water molecule is:
- Correct answer: Polar covalent
- The electronegativity difference between O (3.5) and H (2.1) indicates that the O-H bond is polar covalent. This means there is an unequal sharing of electrons between the atoms, creating partial positive and partial negative charges.

Overall, your answers are correct! Good job.

1) To determine which compound has the largest lattice energy, we need to consider the charges and sizes of the ions involved. Lattice energy is the energy released when gaseous ions combine to form a solid crystal lattice.

In general, lattice energy increases with the charges on the ions and decreases with the size of the ions. Greater charges result in stronger electrostatic attraction, while smaller ions allow for closer proximity and stronger interactions.

In this case, we compare LiF, LiCl, NaF, and NaCl. The charges on the ions are +1 for Li and Na, and -1 for F and Cl. Since all the anions are the same (-1), we only need to consider the cationic charges and sizes.

Li+ is smaller than Na+ because it has fewer energy levels. Comparing the same cation with different anions, the greater the charge on the cation, the stronger the electrostatic attraction. Therefore, LiF has the largest lattice energy among the options given.

So, your answer of LiF having the largest lattice energy is correct.

2) The ionic character in a compound's bonding refers to the extent to which electrons are transferred from one atom to another. Compounds with large differences in electronegativity tend to have more ionic character in their bonding.

In this case, we compare CaBr2, GeBr4, KBr, and GaBr3. We need to consider the electronegativity difference between the cation and anion.

Ca has an electronegativity of 1.0, Ge has an electronegativity of 2.01, K has an electronegativity of 0.82, and Ga has an electronegativity of 1.81. Since Br has an electronegativity of 2.96, we can determine the electronegativity differences for each compound as follows:

CaBr2: |1.0 - 2.96| = 1.96
GeBr4: |2.01 - 2.96| = 0.95
KBr: |0.82 - 2.96| = 2.14
GaBr3: |1.81 - 2.96| = 1.15

The larger the electronegativity difference between the cation and anion, the more ionic character in the bonding. Therefore, KBr has the most ionic character among the options given.

So, your answer of KBr having the most ionic character is correct.

3) To determine which end of the B-N bond is negative, we need to consider the electronegativities of boron (B) and nitrogen (N). Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.

Unfortunately, without access to the specific table on page 364 of your text, I cannot provide the exact electronegativity values. However, in general, nitrogen (N) is more electronegative than boron (B).

The more electronegative element in a bond tends to attract electrons towards itself, resulting in a partial negative charge. Therefore, in the B-N bond, nitrogen (N) would be expected to be more negative than boron (B).

So, your answer of N being the negative end of the B-N bond is correct.

4) To determine the nature of the O-H bond in a water molecule, we need to consider the electronegativity difference between oxygen (O) and hydrogen (H).

Oxygen is more electronegative than hydrogen, meaning it has a greater ability to attract electrons towards itself. In a water molecule (H2O), the oxygen atom pulls the shared electrons closer to itself, resulting in a partial negative charge on oxygen and a partial positive charge on each hydrogen.

A nonpolar covalent bond occurs when the electronegativity difference is very small or nonexistent. An ionic bond occurs when there is a large electronegativity difference and complete transfer of electrons. A polar covalent bond occurs when there is a moderate electronegativity difference and partial transfer of electrons.

Since there is a moderate electronegativity difference between oxygen and hydrogen, the O-H bond in a water molecule is polar covalent.

So, your answer of the O-H bond being polar covalent is correct.