Chapter 5

Question 1

how to determine the formal charge on an atom

Answer 1

atomic number - #valence electrons -nnumber of bonds

Question 2

what does the size of the dipole do

Answer 2

if the larger the dipole, the stronger the harder it is to pull molecules away from eachother. consequenty. the higher the boiling point is

Question 3

resonance structured

Answer 3

different lewis structures for the same compound

Question 4

formal charge

Answer 4

the charge an atom would have in a molecule if all bonds were shared equally

Question 5

the sum of the formal charges is equal to

Answer 5

the charge of the molecule

Question 6

where should the negative formal charges go if they must occur

Answer 6

on the most electronegative element

Question 7

vesper

Answer 7

electrons in one pair or bond repel eachother.

Question 8

electronic geometry

Answer 8

the geometry for all of the electron groups the basic one

Question 9

molecular geometry

Answer 9

the geometry just accounting for the elements this is the complex one

Question 10

4 electron groups eg

Answer 10

tetrahedral 109.5

Question 11

3 electron groupseg

Answer 11

trigonal planar 120

Question 12

2 electron groups eg

Answer 12

linear 180

Question 13

4 electron groups 1 lp mg

Answer 13

trigonal pyramidal <109.5

Question 14

4 electron groups 2 lp mg

Answer 14

bent <109.5

Question 15

how does bond length affect bond angle

Answer 15

as bond length increases the bond angle decreases as elements become easier to move together

Question 16

how does atomic radius affect thebond angle

Answer 16

the larger the atomic radius, the smaller the angle is

Question 17

as a carbon carbon increases in number of bonds what happens

Answer 17

the bond dissociation energy increases and the length decreases

Question 18

Do resonance structures always contribute equally to the overall structure of a molecule? why

Answer 18

no
Just because a molecule can have multiple resonance structures, that does not mean that it is the most desired for the molecule. Molecules tend to prefer smaller or 0 values for the formal charges. On top of that it is best to put the negative formal charge on the most electronegative element.

Question 19

What constitutes an electron group?

Answer 19

Electron groups are defined by as lone pairs, single bonds,multiple bonds, and even single electrons define them. They repel each other through coulombic forces.

Question 20

How do you determine whether a molecule is polar?

Answer 20

1. Determine whether the polar bonds add together to form a net dipole moment.
2. Draw the Lewis structure for the molecule and determine the molecular geometry.
3. Determine whether the molecule contains polar bonds.

Question 21

Which of the two compounds, H2NNH2 and HNNH, has the strongest nitrogen-nitrogen bond, and which has the shorter nitrogen-nitrogen bond.

Answer 21

HNNH has both the strongest nitrogen-nitrogen bond and the shorter nitrogen-nitrogen bond.

the double bond is stronger and shorter

Question 22

what causes bond andgles to deviate

Answer 22

their bond angles should deviate from the idealized bond angle as lone pairs are more repulsive than bonding pairs of electrons. Large atoms, such as Cl or Br, will cause bond angles to deviate from the ideal, and the presence of a multiple bond will cause a deviation as well owing to the increased electron density, so COCl2 should deviate from the idealized bond angle. CH4 has identical atoms symmetrically surrounding a central atom with no lone pairs on it, so CH4 should not deviate from the idealized bond angle.`

Question 23

Which explanation best predicts which species has the smaller bond angle, ClO4− or ClO3−

Answer 23

ClO3− will have the smaller bonding angle since it contains one lone pair of electrons, and lone pair–bonding pair repulsions are greater than bonding pair– bonding pair repulsions.

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