paulpaul

Question 1

They determine the element’s identity

Answer 1

Proton

Question 2

They contribute to the atom’s mass and stability

Answer 2

Neutron

Question 3

They occupy specific energy levels or shells.

Answer 3

Electrons

Question 4

460 BC - Greek philosopher proposes the existence of the atom

Answer 4

Democritus

Question 5

He pounded materials until he made them into smaller and smaller parts

Answer 5

Democritus

Question 6

He called them _____ which is Greek for “_____”.

Answer 6

He called them atomos which is Greek for “indivisible”.

Question 7

1803 - British chemist; elements combine in specific proportions to form compounds

Answer 7

John dalton

Question 8

Solid Sphere Model or Bowling Ball Model

Answer 8

Proposed by John Dalton

Question 9

All substances are made of atoms that cannot be ____, _____, or ____.

Atoms join with _____.

Atoms of the same element are _______, and atoms of different elements are ________.

Answer 9

created, divided, destroyed

other atoms to make new substances.

exactly alike, different in mass and size.

JOHN DALTON

Question 10

1897 - English chemist and physicist; discovered 1st subatomic particles

Answer 10

JJ Thompson

Question 11

Plum Pudding Model or Raisin Bun Model

Answer 11

Proposed by J.J. Thomson

Question 12

Atoms contain negatively charged particles called electrons and positively charged matter called protons.

Created a model to describe the atom as a sphere filled with positive matter with negative particles mixed in

Answer 12

Jj thomson

Question 13

1912 - New Zealand physicist discovered the nucleus

Answer 13

Ernest Rutherford

Question 14

Nuclear Model

Answer 14

Proposed by Ernest Rutherford

Question 15

Small, dense, positively charged particle present in ______ called a ___

_____ travel around the _____, but their exact places cannot be described.

Answer 15

nucleus, proton

electron, nucleus

Ernest rutherford

Question 16

Gold foil experiment

Answer 16

Ernest rutherford

Question 17

1913 - Danish physicist; discovered energy levels

Answer 17

Neil’s Bohr

Question 18

Planetary model

Answer 18

Niels bohr

Question 19

_____ travel around the nucleus in definite paths and fixed distances.

_____ can jump from one level to a path in another level.

Answer 19

Electrons

NIELS BOHR

Question 20

1924 - Austrian physicist; developed the electron cloud model

Answer 20

Erwin Schrodinger

Question 21

Electron Cloud Model

Answer 21

Proposed by Erwin Schrodinger

Question 22

The exact path of ____ cannot be predicted.

The region referred to as the ______, is an area where electrons can likely be found.

Answer 22

Electrons

Electron cloud

Erwin Schrödinger

Question 23

1932 - English physicist; discovered neutrons

Answer 23

James Chadwick

Question 24

_____ have no electrical charge.

Neutrons have a mass nearly equal to the mass of a _____.

Unit of measurement for subatomic particles is the atomic mass unit (____ )

Answer 24

Neutrons

Proton

Amu

Question 25

Proposed by Neils Bohr and Erwin Madelung in 1926. this principle states that electrons in an atom occupy the lowest available energy levels. When building up the electron configuration of an atom, electrons fill the most stable (lowest energy) orbitals first.

Answer 25

Aufbau Principle

Question 26

Formulated by Freidrich Hund in 1925, Hund’s Rule explains how electrons occupy orbitals of equal energy.

When filling orbitals of equal energy, electrons occupy them singly and with parallel spins (same directions) before pairing up.

Electrons will occupy empty orbitals before pairing up in already occupied orbitals.

Answer 26

Hund’s Rule

Question 27

No two electrons in an atom can have the same set of quantum numbers ( n,l,ml,ms)

Answer 27

Pauli’s Exclusion

Question 28

3 Principles in writing electron configuration

Answer 28

Aufbau principle, Hunds rule, Pauli’s exclusion

Question 29

The movement of electrons in 3d space

Spectra of poly electronic atom

Answer 29

Bohrs Atomic Model

Question 30

the set of numbers used to describe the position and energy of the electron in an atom

Answer 30

Quantum numbers

Question 31

The Principal Quantum Numbers (_)

Answer 31

n

Question 32

Angular Momentum Quantum Numbers (__)

Answer 32

(l)

Question 33

Magnetic Quantum Numbers (__)

Answer 33

m l

Question 34

Electron Spin Quantum Numbers

Answer 34

(ms)

Question 35

The Principal Quantum Numbers (n) or

Answer 35

Electron shells)

Question 36

designates the principal electron shell.

It indicates the main energy level occupied by an electron.

Answer 36

The principal quantum numbers

Question 37

Angular Momentum Quantum Numbers (l) or

Answer 37

Sub shells

Question 38

It indicates the shape of the orbital

Answer 38

Angular Momentum Quantum Numbers ( l)
(sub-shells)

Question 39

determines the number of orbitals and their orientation within a subshell.

Answer 39

Magnetic Quantum Numbers (ml)

Question 40

describes the angular momentum of an electron

Answer 40

Electron Spin Quantum Numbers (ms)

Question 41

of an atom is a shorthand method of writing the location of electrons by sublevel.

Answer 41

electron configuration

Question 42

2p^2

Answer 42

2 = energy level
^2 = no. Of electrons
P = energy sublevel

Question 43

The periodic table can be used as a guide for electron configurations.

•The period number is the value of n.
•Groups 1A and 2A have the s-orbital filled.
•Groups 3A - 8A have the p-orbital filled.
•Groups 3B - 2B have the d-orbital filled.
•The lanthanides and actinides have the f-orbital filled

Answer 43

-go girl