Atomic Structure and Arrangement

Question 1

Where was the original idea of the atom from?

Answer 1

Democratitus in Ancient Greece

Question 2

Atomism

Answer 2

Idea by Ancient Greek Leucippus that everything is composed entirely of indivisible elements, called atoms

Question 3

Aristotle’s atomic theory

Answer 3

Believed all substances were a combination of fire, water, earth, and air

Question 4

Dalton’s atomic theory

Answer 4

All matter is made of tiny indivisible particles called atoms, atoms of the same substance are identical, atoms of different elements form in ratios to create compounds, and chemical reactions are the rearranging of atoms

Question 5

J.J Thomson’s atomic experiment

Answer 5

Happened in 1897, used a vacuum tube where gases were placed and an electrical beam went through the tube. He found that with every gas he tested, the ratio of charge to mass was the same, meaning the same pieces were in every atoms

Question 6

Plum pudding atomic model

Answer 6

Made by Thomson, only had electrons that were stuck in positive material

Question 7

Milken’s atomic experiment

Answer 7

Used to find the quantity of charge an electron has

Question 8

Rutherford’s atomic experiment

Answer 8

Performed in 1910, shot alpha particles at gold foil, he expected all the particles to pass through the foil. Some passed through, but others bounced back, showing that the atom had a nucleus.

Question 9

QAM/QMM atomic model

Answer 9

Modern model that says the atom has an electron cloud and a nucleus

Question 10

Electron cloud

Answer 10

Large region where you might find an electron

Question 11

Nucleus

Answer 11

Small, positively charged, and dense, where protons and neutrons are found

Question 12

Proton

Answer 12

Positively charged subatomic particle, +1 charge

Question 13

Neutron

Answer 13

Subatomic particle with no charge

Question 14

Electron

Answer 14

Negatively charged subatomic particle, -1

Question 15

Picometers

Answer 15

Unit of measurement used for atoms

Question 16

Atomic number

Answer 16

Number of protons in an atom, same as the electrons in a neutral atom

Question 17

Mass number

Answer 17

Number of protons + the number of neutrons in an atoms

Question 18

Ion

Answer 18

Atoms with a different number of electrons, making them not neutral anymore

Question 19

Cation

Answer 19

Positively charged ion, where electrons are lost

Question 20

Anion

Answer 20

Negatively charged ion, where electrons are gained

Question 21

Isotope

Answer 21

Atoms with a different number of neutrons, changing the mass number

Question 22

Atomic mass unit (amu)

Answer 22

Unit used to measure how heavy atoms are

Question 23

Ground state

Answer 23

When atoms have their electrons in the lowest energy level possible, ex. hydrogen’s electron in the 1s orbital

Question 24

Excited state

Answer 24

When atoms have their electrons in a higher energy level than normal, ex. hydrogen’s electron in the 2s orbital

Question 25

Principle Atomic Number

Answer 25

Represented with n, the energy level of an electron

Question 26

Atomic orbitals

Answer 26

Differently shaped regions in an atom with a high probability to find an electron

Question 27

S orbitals

Answer 27

In every energy level, holds 2 electrons, holds a max of 2

Question 28

P orbitals

Answer 28

Start at the 2nd energy level, 3 different shapes, each can hold 2, holds a max of 6

Question 29

D orbitals

Answer 29

Start at the 3rd energy level, 5 different shapes, each holding 2, holds a max of 10

Question 30

F orbitals

Answer 30

Start at the 4th energy level, 7 different shapes, each holding 2, holds a max of 14

Question 31

Pauli Exclusion Principle

Answer 31

Says that no 2 electrons can be the same in all ways

Question 32

Hund’s Rule

Answer 32

Idea that electrons fill orbitals of the same energy level, and prefer to fill empty ones first. All 1/2 filled orbitals have the same spin

Question 33

Noble gas configuration

Answer 33

Using noble gases as a shorthand electron configuration, because they have a full outer energy level

Question 34

Lewis diagram

Answer 34

Shows the valence electrons around the symbol of an atom

Question 35

Bohr model

Answer 35

Shows the energy levels and all of the electrons in an atom