Atomic Structure, Electron configuration, and Ionization Energy

Question 1

What is inside the nucleus?

Answer 1

Protons and neutrons

Question 2

What is outside the nucleus

Answer 2

Electrons

Question 3

What subatomic particles have significant weight to them

Answer 3

Protons and Neutrons

Question 4

What are isotopes?

Answer 4

Atoms of the same element with a different # of neutrons/different weights

Question 5

What are ions?

Answer 5

Atoms that have gained or lost an electron and have different charges

Question 6

What are electron configurations used for?

Answer 6

Finding where electrons are in an atom

Question 7

Where can electrons be found?

Answer 7

In different energy levels of clouds/orbitals

Question 8

What are the 4 types of orbitals

Answer 8

S orbital - 1 orbital/2 electrons
P orbital - 3 orbitals/ 6 electrons
D orbital - 5 orbitals/10 electrons
F orbitals - 7 orbitals/ 14 electrons

Question 9

What element types end with S orbitals

Answer 9

Alkali metals, Alkali earth metals, and Helium

Question 10

What element types end with P orbitals

Answer 10

Nonmetals and metalloids

Question 11

What element types end with D orbitals

Answer 11

Transitional metals + Lanthanum and Actinium

Question 12

What element types end with F orbitals

Answer 12

Lanthanoids and Actinoids

Question 13

What is the Aufbau principle

Answer 13

Lower energy levels should be filled before the next higher one (S orbitals first, then P orbitals and so on)

Question 14

What is Hund’s Rule

Answer 14

Electrons fill empty orbitals in parallel directions before filling opposite direction (Similar to how people sit in buses or airplanes)

Question 15

What is the Pauli Exclusion principle

Answer 15

No two electrons can have the same spin direction in an orbit (Only up and down spins)

Question 16

Shortened version used with electron configuration

Answer 16

Using a noble gas (Full orbital) and adding the amount of orbits to get to the element needed (Ex. Rubidium: [Kr] 5s^1)

Question 17

What is ionization energy

Answer 17

The energy needed to remove an electron from an atom or ion

Question 18

“Formula” of removing an electron

Answer 18

Li1 + e- = Li
Li2 + e- = Li1
Li3 + e- = Li2

Question 19

What factors affect ionization energy

Answer 19

Nuclear charge, Atomic radius, and Electron shielding

Question 20

Electron shielding

Answer 20

Electrons in sub levels lower than the valence electrons repelling them more than protons in the nucleus can attract (decreases IE)

Question 21

Valence electrons

Answer 21

Electrons in the last shell of an atom

Question 22

Atomic Radius

Answer 22

Howe many energy levels or “rings” the atom has that increases down a column (Decreases IE)

Question 23

Nuclear charge

Answer 23

How many protons an atom has (increases IE)

Question 24

Why does Ionic energy decrease for each noble gas

Answer 24

Because the farther down the column of noble gases, the larger the atomic radius and the less that protons have an effect on electrons (Atomic radius, Electron shielding)