Chapter 1: Atomic Structure

Question 1

Principle Quantum Number

Answer 1

n
Describes the average energy and the shell, shape.

Higher n= higher energy level= greater radius.

Question 2

Azimuthal Quantum Number

Answer 2

l
describes the subshells within a given principle energy level (s,p,d, and f).

Question 3

Magnetic Quantum Number

Answer 3

ml
specifies the orbital within a subshell where an electron can be located

Question 4

Spin Quantum Number

Answer 4

ms
Designates the spin orientation (+-1/2) of an electron orbital.

Question 5

l=0 subshell

Answer 5

s

Question 6

l=1 subshell

Answer 6

p

Question 7

l=2 subshell

Answer 7

d

Question 8

l=3 subshell

Answer 8

f

Question 9

Maximum number of electrons in orbital

Answer 9

2 electrons

Question 10

Maximum number of electrons in subshell

Answer 10

4l+2

Question 11

How many orbitals in s?

Answer 11

1 orbital

Question 12

How many orbitals in p?

Answer 12

3 orbitals

Question 13

How many orbitals in d?

Answer 13

5 orbitals

Question 14

How many orbitals in f?

Answer 14

7 orbitals

Question 15

Quantum

Answer 15

The energy difference between energy levels

Question 16

Ground State

Answer 16

the lowest energy state, the energy of the ground state is known as the zero-point energy of the system, the state in which all e-s are in lowest possible orbitals

Question 17

Excited State

Answer 17

A state in which at least one e- has moved to a subshell of higher than normal energy

Question 18

As electrons go from a lower energy level to a higher energy level, they…

Answer 18

…get AHED:
Absorb Light
Higher potential
Excited
Distant (from the nucleus)

Question 19

Lyman Series

Answer 19

the group of hydrogen emission lines corresponding to transition from energy levels n>2 to n=1

Question 20

Balmer Series

Answer 20

the group corresponding to transition from energy levels n>3 to n=2 and includes four wavelengths in the visible region (the shorter photon wavelengths in the UV region).

Question 21

Paschen Series

Answer 21

corresponds to transition from n>4 to n=3.

Question 22

Orbitals

Answer 22

The localized regions of space that electrons are likely to be found in.

Question 23

Heisenberg uncertainty principle

Answer 23

It is impossible to simultaneously know both the location and momentum of an electron.

Question 24

Pauli exclusion principle

Answer 24

no two electrons in a given atom can posses the same set of four quantum numbers.

Question 25

Aufbau principle

Answer 25

aka building-up principle. Electrons fill from lower to higher energy subshells and each subshell will completely fill before electrons enter the next one.

Question 26

Hund's rule

Answer 26

subshells with multiple orbitals fill electrons so there is a maximum number of 1/2 filled orbitals first because of electron repulsion

Question 27

Exceptions to electron configuration?

Answer 27

Chromium (Z=24) Copper (Z=29) Chromium should have EC: [Ar]4s2 3d4 Instead has = [Ar]4s1 3d5 Copper should have EC: [Ar] 4s2 3d9 Instead has: [Ar] 4s1 3d10 stability of full d or f shell outweighs the energetically unfavorable cost of removing an electron from an s orbital. Doesn't work for p subshell.

Question 28

Paramagnetic materials

Answer 28

Materials that have unpaired electrons that align with the magnetic field, attracting the material to the magnet.

Question 29

Diamagnetic

Answer 29

Materials that have all paired electrons, which can not be easily realigned; they are repelled by magnets.