Electron Configuration

Question 1

period

Answer 1

row of periodic table

Question 2

What does the period number correspond to?

Answer 2

principle energy level

Question 3

group

Answer 3

column of periodic table

Question 4

What does the group number correspond to?

Answer 4

number of electrons in valence level

Question 5

What is electron configuration based on?

Answer 5

Quantum Mechanical Model

Question 6

What will electrons in the ground state occupy?

Answer 6

lowest possible energy level

Question 7

What can electrons only have?

Answer 7

specific energy levels

Question 8

What is each energy level split into?

Answer 8

sublevels

Question 9

Are all sublevels available at every energy level?

Answer 9

no

Question 10

What are sublevel made up of?

Answer 10

a number of possible orbitals

Question 11

What does each orbial have?

Answer 11

identical energy

Question 12

How many possible orbitals does the s sublevel have?

Answer 12

1

Question 13

How many possible orbitals does the p sublevel have?

Answer 13

3

Question 14

How many possible orbitals does the d sublevel have?

Answer 14

5

Question 15

How many possible orbitals does the f sublevel have?

Answer 15

7

Question 16

What does each orbital represent?

Answer 16

a region in space with 90% chance of finding a specific electron

Question 17

How many electrons can occupy any specific orbital?

Answer 17

maximum 2 electrons

Question 18

Describe the s sublevel.

Answer 18

1 orbital

spherical

Question 19

Desribe the p sublevel.

Answer 19

3 orbitals

dumbell shaped

Question 20

Aufbau principle

Answer 20

gives order of electron configuration

Question 21

Hund Rule

Answer 21

gives half fill identical orbitals then pair up electrons

Question 22

Pauli Exclusion

Answer 22

no 2 electrons can be identical

Question 23

What does Z = x mean?

Answer 23

atom has x electrons

Question 24

What must be done when drawing energy level diagrams for 3d and 4s?

Answer 24

Put overlap

Question 25

1st ionization energy

Answer 25

energy needed to remove 1 mol of electrons from 1 mol of atoms in gaseous state

removal of electron in highest energy level to infinity

Question 26

How can first ionization energy be calculated?

Answer 26

from wavelength or frequency of convergence limit

Question 27

successive energy level

Answer 27

energy needed to remove next mol of electrons then next and next

Question 28

What does the energy needed to remove specific electron depend on?

Answer 28

nuclear charge (higher charge, more attraction to nucleus)

distance from nucleus (further away, less attraction)

shielding (full sublevels shild outermost electron, less attraction)

Question 29

What are the two exceptions to the Aufbau Principle?

Answer 29

Cr [Ar] 4s¹ 3d⁵

Cu [Ar] 4s¹ 3d¹⁰

because s electron moves to d sublevel

more stable

Question 30

What is the convergence level shown to be?

Answer 30

wavelength = x

Question 31

convergence limit

Answer 31

where energy levels run out

Question 32

What is the formula for the first ionization energy?

Answer 32

E = hc/x

Question 33

What does the energy of photon correspond to?

Answer 33

first ionization energy

Question 34

uncertainty principle

Answer 34

cannot know where an electron is at any given moment in time but can work out where electron likely to be

Question 36

atomic orbital

Answer 36

region around an atomic nucleus with a 90% probability of finding an electron

Question 37

Why can electrons occupy same region of space despite mutual repulsion?

Answer 37

spin in opposite directions

Question 38

electron configuration for Cr

Answer 38

Cr: [Ar] 3d⁵ 4s¹

Question 39

electron configuration for Cu

Answer 39

Cu: [Ar] 3d¹⁰ 4s¹

Question 40

Why do chromium and copper have different electron configurations?

Answer 40

half-full (or full) d sublevel relatively stable because minimizes electron repulsion with six singly occupied orbitals (or all orbitals filled)

Question 41

What is the equation for the first ionization energy of hydrogen?

Answer 41

H(g) -> H⁺ + e^-