Basics

Question 1

Periods

Answer 1

Rows on the Periodic Table

Question 2

Groups

Answer 2

Columns on the Periodic Table

Question 3

Group 1

Answer 3

Alkaline Metals

Question 4

Group 2

Answer 4

Alkaline Earth Metals

Question 5

Group 7

Answer 5

Halogens

Question 6

Group 8

Answer 6

Noble Gases

Question 7

Electronegativity Trend

Answer 7

Increases up and to the right (towards Fluorine the most EN element)

Question 8

Electronegativity

Answer 8

Is a measure of the tendency of an atom to attract a bonding pair of electron; How badly it wants an electron

Question 9

Size / Atomic Radius Trend

Answer 9

Increases down (increasing orbitals and shells)
Increases left (decreased pull of electrons toward the nucleus)

Question 10

Ionization Energy

Answer 10

The energy required to remove an electron from the outer shell of a gaseous atom or ion

Question 11

Ionization Energy Trend

Answer 11

Increases Up and to the Right

Question 12

Effective Nuclear Charge (Zeff)

Answer 12

The attractive positive charge of nuclear protons acting on valence electrons

Question 13

Zeff Trend

Answer 13

Increases to the Right (electrons pulled in closer to nucleus)

Question 14

Electron Affinity

Answer 14

The amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion

Question 15

Electron Affinity Trend

Answer 15

Increases Up and to the Right (affinity becomes less negative)

Question 16

Speed of Light (C)

Answer 16

3 x 10 ^ (8) m/s

Question 17

Planck’s Constant (J)

Answer 17

6.6 x 10 ^ (-34) J x S

Question 18

Electron Configuration

Answer 18

Where the electrons are (orbitals)

Ex: 1s^(2) 2S^(2) 2p^(6)

Question 19

Aufbau Principle

Answer 19

“Build up rule” begin with low energy orbitals and move to higher energy orbitals

Question 20

Hunds Rule

Answer 20

One electron goes in each suborbital before doubling them up

Question 21

Pauli Exclusion Principle

Answer 21

No two electrons can have the same 4 quantum numbers

Question 22

Principle Quantum Number (n)

Answer 22

Energy Level; Period in the periodic table

2n^2 = maximum number of electrons in level “n”

Question 23

Azimuthal Quantum Number (L)

Answer 23

Orbital; Shape
0=S
1=p
2=d
3=f

4L+2 = electrons per orbital

Question 24

Magnetic Quantum Number (M L)

Answer 24

Sub-Orbital (-L to +L)

Question 25

Spin Quantum Number (M s)

Answer 25

Direction of electron (+ 1/2 or - 1/2)

Question 26

Protium

Answer 26

Isotope of Hydrogen with 1 proton and 0 neutrons = mass of 1amu

Question 27

Deuterium

Answer 27

Isotope of Hydrogen with 1 proton and 1 neutron = mass of 2amu

Question 28

Tritium

Answer 28

Isotope of Hydrogen with 1 proton and 2 neutron = mass of 3amu

Question 29

Isotope

Answer 29

Different weight for the same element (protons remain the same and the # of neutrons changes)

Question 30

Average Mass Formula

Answer 30

Avg. Mass = (Isotope x (% abundance / 100)) + (Isotope x (% abundance / 100)) + ….