Polarity and Geometry of SBr2

Polarity and Geometry of SBr2

Assessment

Interactive Video

Chemistry

10th - 12th Grade

Practice Problem

Hard

Created by

Sophia Harris

FREE Resource

The video tutorial explores whether SBr2 is polar or nonpolar. It begins by identifying bromine and sulfur as nonmetals, forming a molecular compound. The electronegativity values of sulfur (2.58) and bromine (2.96) are compared, showing a difference of less than 0.5, indicating a nonpolar compound. The molecular geometry is examined, revealing a bent shape due to lone pairs, causing a slight dipole. However, the difference in electronegativity is insufficient to make SBr2 polar. The conclusion reaffirms SBr2 as nonpolar covalent due to the small electronegativity difference.

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9 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What type of elements are sulfur and bromine in the context of SBr2?

Metalloids

Nonmetals

Metals

Noble gases

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the electronegativity value of sulfur?

2.96

1.90

3.44

2.58

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

According to the rule of thumb, what electronegativity difference indicates a nonpolar compound?

Between 0.5 and 1.0

Exactly 0.5

Greater than 1.0

Less than 0.5

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the molecular geometry of SBr2?

Trigonal planar

Tetrahedral

Linear

Bent

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How do lone pairs affect the shape of the SBr2 molecule?

They make it linear

They make it trigonal planar

They have no effect

They cause a bent shape

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Why does SBr2 have a slight dipole moment?

Due to equal electronegativity

Because of lone pairs

Due to a difference in electronegativity

Because of its linear shape

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Despite having a slight dipole, why is SBr2 considered nonpolar?

It has a linear shape

The electronegativity difference is less than 0.5

The dipole is too strong

It has no lone pairs

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