Exam 3 Review

Question 1

What is the formula for wavelength?

Answer 1

λ = c / f

Question 2

What is c?

Answer 2

c is the speed of light (approximately 3.00 x 10^8 m/s)

Question 3

What is f?

Answer 3

f is the frequency in Hertz (Hz)

Question 4

How do you convert m to nm?

Answer 4

1 m x 10^9 nm

Question 5

How do you calculate energy of a photon?

Answer 5

E = hc/λ

Question 6

What is h?

Answer 6

Planck’s constant.

Question 7

What is Planck’s constant?

Answer 7

6.626 × 10^-34 J·s

Question 8

What is c?

Answer 8

3.00x10^8

Question 9

What is the Rhydberg equation?

Answer 9

ΔE = -RH (1/nf^2 - 1/ni^2)

Question 10

What is RH?

Answer 10

RH = 2.179 × 10 ^ -18 J

Question 11

What is l for s orbitals?

Answer 11

0

Question 12

What is l for p orbitals?

Answer 12

1

Question 13

What is l for d orbitals?

Answer 13

2

Question 14

What is l for f orbitals?

Answer 14

3

Question 15

When does effective nuclear charge increase?

Answer 15

Effective nuclear charge increases across a row due to increasing number of protons.

Question 16

When does electron shielding occur?

Answer 16

Electron shielding occurs when inner energy levels disrupt attractive forces between the nucleus and the electrons in the outer energy level.

Question 17

What is atomic radius?

Answer 17

The size of the atom.

Question 18

When does atomic radius decrease?

Answer 18

It decreases across a row left to right due to increased nuclear charge pulling valence electrons in outer energy level closer to the nucleus.

Question 19

When does atomic radius increase?

Answer 19

Radius increases down a row due to increased shielding, reducing attraction of valence electrons to nucleus and making atom larger.

Question 20

What is ionization energy?

Answer 20

Ionization energy is energy required to remove an electron from an atom.

Question 21

When does ionization energy decrease?

Answer 21

It decreases down a row due to electron shielding.

Question 22

When does ionization energy increase?

Answer 22

It increases going across a row due to increased nuclear charge.

Question 23

What is electron affinity?

Answer 23

Electron affinity is energy released when an atom adds an electron.

Question 24

When does electron affinity increase?

Answer 24

It increases going across a row.

Question 25

When does electron affinity decrease?

Answer 25

It decreases going down a column.

Question 26

Which bonds are sigma bonds?

Answer 26

The first bond.

Question 27

What are pi bonds?

Answer 27

The following bonds.

Question 28

What is the bond order?

Answer 28

Total number of bonds.

Question 29

How to find valence electrons?

Answer 29

Count how many over the element is. If there is a positive charge, deduct that number of electrons. If there is a negative charge, add that number of electrons.

Question 30

What makes bond energy high?

Answer 30

More bonds.

Question 31

What makes bond energy low?

Answer 31

Less bonds.

Question 32

What makes bond length high?

Answer 32

Less bonds.

Question 33

What makes bond length low?

Answer 33

More bonds.

Question 34

What are the electron domains?

Answer 34

The total number of bonding pairs and lone pairs in a molecule.

Question 35

How to find hybridization?

Answer 35

It’s always dependent on the number of electron domains.

Question 36

What does it mean when the electron pair geometry is linear?

Answer 36

There are 2 domains.

Question 37

What does it mean when the electron pair geometry is trigonal planar?

Answer 37

There are 3 domains.

Question 38

What does it mean when the electron pair geometry is tetrahedral?

Answer 38

There are 4 domains.

Question 39

What does it mean when the electron pair geometry is trigonal bipyramidal?

Answer 39

There are 5 domains.

Question 40

What does it mean when the electron pair geometry is octahedral?

Answer 40

There are 6 domains.

Question 41

What does it mean when molecular geometry is linear?

Answer 41

There are 2 bonding pairs.

Question 42

What does it mean when molecular geometry is trigonal planar?

Answer 42

There are 3 bonding pairs.

Question 43

What does it mean when molecular geometry is bent?

Answer 43

There are 2 bonding pairs and 1 lone pair or 2 bonding pairs and 2 lone pairs.

Question 44

What does it mean when molecular geometry is trigonal pyramidal?

Answer 44

There are 3 bonding pairs and 1 lone pair.

Question 45

What does it mean when 5 domain molecular geometry is see saw?

Answer 45

There are 5 bonding pairs.

Question 46

What does it mean when 5 domain molecular geometry is t-shaped?

Answer 46

There are 3 bonding pairs and 2 lone pairs.

Question 47

What does it mean when 5 domain molecular geometry is linear?

Answer 47

There are 2 bonding pairs and 3 lone pairs.

Question 48

What does it mean when 6 domain molecular geometry is octahedral?

Answer 48

There are 6 bonding pairs.

Question 49

What does it mean when 6 domain molecular geometry is square pyramidal?

Answer 49

There are 5 bonding pairs and 1 lone pair.

Question 50

What does it mean when 6 domain molecular geometry is square planar?

Answer 50

There are 4 bonding pairs and 2 lone pairs.

Question 51

What are dispersion forces?

Answer 51

A nonpolar particle can be temporarily polarized to create dispersion force.

Question 52

What are dipole-dipole interactions?

Answer 52

Polar molecules have a more positive and a more negative end—a dipole. The oppositely charged ends attract each other.

Question 53

What are hydrogen bonds?

Answer 53

A hydrogen bond is an attraction between a hydrogen atom attached to a highly electronegative atom and a nearby small electronegative atom in another molecule or chemical group.

Question 54

What elements can form a hydrogen bond?

Answer 54

Hydrogen bonding arises in part from the high electronegativity of nitrogen, oxygen, and fluorine.

Question 55

What does it mean for a molecule to be polar?

Answer 55

It’s bond dipoles are not symmetrical.

Question 56

What does it mean for a molecule to be nonpolar?

Answer 56

The bond dipoles cancel, i.e., equal and/or arranged symmetrically around the center.