Exam 4

Question 1

How was the periodic table organized

Answer 1

its sorted based on atomic mass (number of protons)

Question 2

nuclear charge and its relationship to the periodic table

Answer 2

The force of the electrons reacting with the force of the positive nuclease combines to create the nuclear charge

Increases from left to right in a period

slightly increases as you move down a group but not as much

Question 3

equation for effective nuclear charge(Zeff)

Answer 3

atomic number - # of core electrons

Question 4

How to find bonding atomic radius and the bonding atomic radius relationship to periodic table

Answer 4

half of the distance between the two bonded nuclei

Increases from right to left
increases as you move down a group

Question 5

how does atomic size vary on the periodic table

Answer 5

increases as you move right to left
increases down the group

Question 6

Hybridization that corresponds to an ED of 2

Answer 6

sp

Question 7

Hybridization that corresponds to an ED of 3

Answer 7

sp^2

Question 8

Hybridization that corresponds to an ED of 4

Answer 8

sp^3

Question 9

Hybridization that corresponds to an ED of 5

Answer 9

sp^3d

Question 10

Hybridization that corresponds to an ED of 6

Answer 10

sp^3d^2

Question 11

2 bonds and no lone pairs

Answer 11

Electron geometry: Linear
Molecular geometry: Linear

Question 12

3 bonds and no lone pairs

Answer 12

Electron geometry: trigonal planar
Molecular geometry: trigonal planar

Question 13

2 bonds and 1 lone pairs

Answer 13

Electron geometry: trigonal planar
Molecular geometry: bent

Question 14

4 bonds and no lone pairs

Answer 14

Electron geometry: tetrahedral
Molecular geometry: tetrahedral

Question 15

3 bonds and 1 lone pairs

Answer 15

Electron geometry: tetrahedral
Molecular geometry: trigonal pyramidal

Question 16

2 bonds and 2 lone pairs

Answer 16

Electron geometry: tetrahedral
Molecular geometry: bent

Question 17

5 bonds and no lone pairs

Answer 17

Electron geometry: trigonal bipyramidal
Molecular geometry: trigonal bipyramidal

Question 18

4 bonds and 1 lone pairs

Answer 18

Electron geometry: trigonal bipyramidal
Molecular geometry: seesaw

Question 19

3 bonds and 2 lone pairs

Answer 19

Electron geometry: trigonal bipyramidal
Molecular geometry: T-shaped

Question 20

2 bonds and 3 lone pairs

Answer 20

Electron geometry: trigonal bipyramidal
Molecular geometry: Linear

Question 21

6 bonds and no lone pairs

Answer 21

Electron geometry: octahedral
Molecular geometry: octahedral

Question 22

5 bonds and 1 lone pairs

Answer 22

Electron geometry: octahedral
Molecular geometry: square pyramidal

Question 23

4 bonds and 2 lone pairs

Answer 23

Electron geometry: octahedral
Molecular geometry: square planar

Question 24

3 bonds and 2 lone pairs

Answer 24

Electron geometry: octahedral
Molecular geometry: T-shaped

Question 25

Equation for formal charge

Answer 25

Valence - (bonding pairs/2) - lone pair electrons (individual electrons)

Question 26

rules for picking formal charge

Answer 26

pick formal charge that has each one closest to 0 Pick the formal charge that best represents an atoms electronegativity relative to other atoms

Question 27

How to rank lattice energy

Answer 27

First rank based on charge (higher overall charges higher lattice energy) Then focus on atomic radius (smaller radius higher lattice energy)

Question 28

How do bond angles correspond to electron geometry

Answer 28

Linear: 180 Trigonal planar: 120 tetrahedral: 109.5 trigonal bipyramidal: 90,120 octahedral: 90 *note that for every lone pair in an electron geometry this slightly decreases the size of the bond angle

Question 29

Paramagnetic vs diamagnetic

Answer 29

Paramagnetic: unpaired electrons diamagnetic: 0 unpaired electrons

Question 30

How does ionization energy change across the periodic table

Answer 30

increases as you move up a group and increases as you move left to right *this is because of the way that effective nuclear charge changes

Question 31

Isoelectronic

Answer 31

two atoms, ions, or molecules that have the same electronic structure

Question 32

How can protons affect core electron orbitals

Answer 32

The positively charged core can pull on the orbitals meaning a larger amount of protons can lead to a smaller orbital

Question 33

Electron shielding

Answer 33

Inner shell electrons will partially block the force of the nucleus on outer shell electrons

Question 34

Bond order

Answer 34

single: 1 double: 2 triple: 3 *for resonance structures, the bond order is an average of all of the bond orders involved in the resonance structure