QuestionWhich bond has the greatest ionic character?
1. $\mathrm{H}-\mathrm{Cl}$
2. $\mathrm{H}-\mathrm{F}$
3. $\mathrm{H}-\mathrm{O}$
4. $\mathrm{H}-\mathrm{N}$

Studdy Solution

STEP 1

What is this asking? Which bond is the most ionic?
Ionic character relates to how different the electronegativities of the atoms are. Watch out! Don't just guess!
We need to actually compare the electronegativity differences.

STEP 2

1. Electronegativity Values
2. Differences in Electronegativity

STEP 3

Let's grab our handy dandy electronegativity table!
We're going to need the electronegativity values for hydrogen ( $H$ ), fluorine ( $F$ ), chlorine ( $Cl$ ), oxygen ( $O$ ), and nitrogen ( $N$ ).

STEP 4

Looking them up, we find: $H = \bold{2.20}$ $F = \bold{3.98}$ $Cl = \bold{3.16}$ $O = \bold{3.44}$ $N = \bold{3.04}$

STEP 5

Now, let's calculate the electronegativity difference for each bond.
Remember, we're looking for the largest difference, because that means the electrons are being hogged more by one atom, making it more ionic!

STEP 6

For $H-F$ : $\lvert 3.98 - 2.20 \rvert = \bold{1.78}$

STEP 7

For $H-Cl$ : $\lvert 3.16 - 2.20 \rvert = \bold{0.96}$

STEP 8

For $H-O$ : $\lvert 3.44 - 2.20 \rvert = \bold{1.24}$

STEP 9

For $H-N$ : $\lvert 3.04 - 2.20 \rvert = \bold{0.84}$

STEP 10

Comparing our differences, we see that $H-F$ has the biggest difference at $\bold{1.78}$ !

STEP 11

The $H-F$ bond has the greatest ionic character!

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QuestionWhich bond has the greatest ionic character?
1. $\mathrm{H}-\mathrm{Cl}$
2. $\mathrm{H}-\mathrm{F}$
3. $\mathrm{H}-\mathrm{O}$
4. $\mathrm{H}-\mathrm{N}$

Studdy Solution

STEP 1

What is this asking? Which bond is the most ionic?
Ionic character relates to how different the electronegativities of the atoms are. Watch out! Don't just guess!
We need to actually compare the electronegativity differences.

STEP 2

1. Electronegativity Values
2. Differences in Electronegativity

STEP 3

Let's grab our handy dandy electronegativity table!
We're going to need the electronegativity values for hydrogen ( $H$ ), fluorine ( $F$ ), chlorine ( $Cl$ ), oxygen ( $O$ ), and nitrogen ( $N$ ).

STEP 4

Looking them up, we find: $H = \bold{2.20}$ $F = \bold{3.98}$ $Cl = \bold{3.16}$ $O = \bold{3.44}$ $N = \bold{3.04}$

STEP 5

Now, let's calculate the electronegativity difference for each bond.
Remember, we're looking for the largest difference, because that means the electrons are being hogged more by one atom, making it more ionic!

STEP 6

For $H-F$ : $\lvert 3.98 - 2.20 \rvert = \bold{1.78}$

STEP 7

For $H-Cl$ : $\lvert 3.16 - 2.20 \rvert = \bold{0.96}$

STEP 8

For $H-O$ : $\lvert 3.44 - 2.20 \rvert = \bold{1.24}$

STEP 9

For $H-N$ : $\lvert 3.04 - 2.20 \rvert = \bold{0.84}$

STEP 10

Comparing our differences, we see that $H-F$ has the biggest difference at $\bold{1.78}$ !

STEP 11

The $H-F$ bond has the greatest ionic character!

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QuestionWhich bond has the greatest ionic character?1. H−Cl\mathrm{H}-\mathrm{Cl}H−Cl2. H−F\mathrm{H}-\mathrm{F}H−F3. H−O\mathrm{H}-\mathrm{O}H−O4. H−N\mathrm{H}-\mathrm{N}H−N

Studdy Solution

STEP 1

What is this asking? Which bond is the *most* ionic?Ionic character relates to how different the electronegativities of the atoms are. Watch out! Don't just guess!We need to actually *compare* the electronegativity differences.

STEP 2

1. Electronegativity Values2. Differences in Electronegativity

STEP 3

Let's **grab our handy dandy electronegativity table**!We're going to need the electronegativity values for hydrogen (HHH), fluorine (FFF), chlorine (ClClCl), oxygen (OOO), and nitrogen (NNN).

STEP 4

Looking them up, we find: H=2.20H = \bold{2.20}H=2.20 F=3.98F = \bold{3.98}F=3.98Cl=3.16Cl = \bold{3.16}Cl=3.16O=3.44O = \bold{3.44}O=3.44N=3.04N = \bold{3.04}N=3.04

STEP 5

Now, let's **calculate the electronegativity difference** for each bond.Remember, we're looking for the *largest* difference, because that means the electrons are being hogged more by one atom, making it more ionic!

STEP 6

For H−FH-FH−F: ∣3.98−2.20∣=1.78\lvert 3.98 - 2.20 \rvert = \bold{1.78}∣3.98−2.20∣=1.78

STEP 7

For H−ClH-ClH−Cl: ∣3.16−2.20∣=0.96\lvert 3.16 - 2.20 \rvert = \bold{0.96}∣3.16−2.20∣=0.96

STEP 8

For H−OH-OH−O: ∣3.44−2.20∣=1.24\lvert 3.44 - 2.20 \rvert = \bold{1.24}∣3.44−2.20∣=1.24

STEP 9

For H−NH-NH−N: ∣3.04−2.20∣=0.84\lvert 3.04 - 2.20 \rvert = \bold{0.84}∣3.04−2.20∣=0.84

STEP 10

Comparing our differences, we see that H−FH-FH−F has the **biggest difference** at 1.78\bold{1.78}1.78!

STEP 11

The H−FH-FH−F bond has the greatest ionic character!

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QuestionWhich bond has the greatest ionic character?
1. $\mathrm{H}-\mathrm{Cl}$
2. $\mathrm{H}-\mathrm{F}$
3. $\mathrm{H}-\mathrm{O}$
4. $\mathrm{H}-\mathrm{N}$

What is this asking? Which bond is the most ionic?
Ionic character relates to how different the electronegativities of the atoms are. Watch out! Don't just guess!
We need to actually compare the electronegativity differences.

1. Electronegativity Values
2. Differences in Electronegativity

Let's grab our handy dandy electronegativity table!
We're going to need the electronegativity values for hydrogen ( $H$ ), fluorine ( $F$ ), chlorine ( $Cl$ ), oxygen ( $O$ ), and nitrogen ( $N$ ).

Looking them up, we find: $H = \bold{2.20}$ $F = \bold{3.98}$ $Cl = \bold{3.16}$ $O = \bold{3.44}$ $N = \bold{3.04}$

Now, let's calculate the electronegativity difference for each bond.
Remember, we're looking for the largest difference, because that means the electrons are being hogged more by one atom, making it more ionic!

For $H-F$ : $\lvert 3.98 - 2.20 \rvert = \bold{1.78}$

For $H-Cl$ : $\lvert 3.16 - 2.20 \rvert = \bold{0.96}$

For $H-O$ : $\lvert 3.44 - 2.20 \rvert = \bold{1.24}$

For $H-N$ : $\lvert 3.04 - 2.20 \rvert = \bold{0.84}$

Comparing our differences, we see that $H-F$ has the biggest difference at $\bold{1.78}$ !

The $H-F$ bond has the greatest ionic character!