Chapter 7 - Atomic Structure and Periodicity

Question 1

Coulomb’s law

Answer 1

F=k((Q1 x Q2)/r^2)
Describes atomic radius size as a function of forces of attraction and repulsion between the nucleus and electrons and electrons and electrons, (shielding and different sized outer oribts of elements given same energy levels)

Question 2

Hund’s rule

Answer 2

schoolbus rule, orbitals fill first half all the way through subshell until filled with half filled orbitals (in 2p, every orbital gets an “up” electron before any “down” electrons appear in any orbital)

Question 3

Pauli Exclusion Principle

Answer 3

No two electrons in the same orbit, position, and orbital can have the same spin (arrow up and arrow down per box)

Question 4

Aufbau Principle

Answer 4

Electrons fill in lowest energy level first (1s first, then 2s)

Question 5

Electronegativity trend (give directions ex. left and down)

Answer 5

Right and up

Question 6

Atomic size trend (give directions (ex. left and down are larger))

Answer 6

Left and down are larger

Question 7

Does effective nuclear charge change as it moves down a group? Why?

Answer 7

No, as the same amount of valence electrons exist for each atom down a group. ( weirdly, as the electrons are still further away, down a group decreases electron affinity/binding energy even though the effective nuclear charge is technically the same (text for clarification if this is too confusing))

Question 8

Order for determining an elements atomic size

Answer 8

1. Energy level
   a. Whether or not there are the same amount of full electron “shields”
2. Amount of protons
   a. And effective nuclear charge acting on valence electrons
3. Amount of valence electrons
   a. Electrons repel, protons in nucleus are less effective and attraction is more spread out thus making it bigger
   4.

Question 9

Metals are more prone to ______ electrons, whereas nonmetals usually _____ electrons. (gain, lose)

Answer 9

1. lose
2. gain

Question 10

Cations are _____ than their original element, whereas anions are _____. Additionally, when a cation and anion are isoelectronic, the cation is substantially smaller. Why is this? (larger, smaller)

Answer 10

1. smaller
2. larger
   because cations lose and electron, therefore decreasing electron-electron repulsion, whereas anions gain an electron, having the opposite effect. When isoelectronic, the cation has a much higher Zeff value (effective nuclear charge), increasing attraction and decreasing distance by Coulomb’s law.

Question 11

Define isoelectronic

Answer 11

Having the same number of electrons (though often not protons)

Question 12

In what direction does electron affinity increase? (ex. top left to bottom right)

Answer 12

up and to the right

Question 13

Electronegativity

Answer 13

The tendency to pull on an electron in a bond

Question 14

What changes going right on the periodic table? What changes moving down?

Answer 14

Effective nuclear charge increases right, energy level and thus shielding increases down

Question 15

Where do metallic and nonmetallic character increase/decrease?

Answer 15

Metallic character increases inversely to nonmetallic character down and left

Question 16

Principal quantum number represents

Answer 16

Shell/energy level (n)

Question 17

Angular momentum quantum number represents:

Answer 17

Subshell/sublevel (n-1= l) (ex. p subshell, s subshell, d subshell)

Question 18

Magnetic quantum number represents:

Answer 18

Orientations (ex. x-y, x-z, y-z)

Question 19

Electron spin quantum number

Answer 19

Determines which way an electron spins (up or down)

Question 20

define degenerate orbitals

Answer 20

oribitals which share the same energy level (the three orbitals in 2p are degenerate with each other)

Question 21

Equation for change in energy (delta E)

Answer 21

Delta E = hv

h = 6.626 x 10^-34
v = frequency

Question 22

de broglies equation

Answer 22

lambda = h/mv

h= 6.626 x 10^-34
m = mass in kg

Question 23

Lyman series (H)

Answer 23

UV
122 nm, 103 nm, 97 nm, 95 nm, 94 nm
90-130

Question 24

Balmer series (H)

Answer 24

visible
656 nm, 486 nm, 434 nm, 410 nm
400-700

Question 25

Paschen series (H)

Answer 25

infrared
1875 nm, 1282 nm, 1094 nm
1000-1900

Question 26

Radio wavelengths:

Answer 26

more than 1 m

Question 27

Microwave wavelengths

Answer 27

between 1 mm to 1 m

Question 28

Infrared wavelengths

Answer 28

700 nm to 1 mm

Question 29

visible wavelengths

Answer 29

400-700 nm

Question 30

x-ray wavelengths

Answer 30

.01-10 nm

Question 31

gamma rays

Answer 31

smaller than .01 nm

Question 32

uv wavelengths

Answer 32

10-400 nm

Question 33

c=

Answer 33

c= lambda v