chem h unit 3

Question 0

Cathode ray –

Answer 0

Thomson’s experiment that was used to support the idea of electrons. The negatively charged electrons were deflected toward the positive end of the magnet.

Question 1

1904 – JJ Thomson’s Model

Answer 1

●Plum Pudding Model (or Chocolate Chip Cookie Model)

●His Theory: The majority of the atom is positively charged, and the electrons are embedded in the positive “core”.

Question 2

1911 – Rutherford’s Model

Answer 2

●His Theory:  He identified the
nucleus and said that it
was positively charged.  
He also said that the
electrons were randomly
placed around the outside
of the nucleus

Question 3

1913 – Bohr’s Model

Answer 3

●His Theory – He added to Rutherford’s model by including neutrons in the nucleus as well as stating that the electrons were traveling in fixed orbits around the nucleus (like planets around the sun)

Question 4

1928 – Electron Cloud Model

Answer 4

●This model is the currently accepted model.
●EXTREMELY small, heavy nucleus that contains the protons and neutrons
●Electrons are very small and light and they travel around the nucleus randomly within energy levels but not in a fixed path

Question 5

PROTONS

Answer 5

Positive

Nucleus

Question 6

Neutrons

Answer 6

Neutral nucleus

Question 7

Electrons

Answer 7

Negative move in space around nucleus

Question 8

Protons and neutrons are about

Answer 8

10,000 times bigger than electrons

Question 9

If you draw an line across the diameter of a penny, there are

Answer 9

810,000,000 atoms of Copper

Question 10

Atomic Number -

Answer 10

The number of protons
in the nucleus
•Every element on
the Periodic Table has
an unique atomic
number

Question 11

Mass number

Answer 11

The number of protons and neutrons

Question 12

Positively charged atoms are equal to

Answer 12

Negatively charged atoms

Question 13

Ions

Answer 13

Ions
What atoms turn into when they gain or lose electrons

•To find the charge on an ion, compare the # of protons to the # of electrons

Question 14

Isotopes -

Answer 14

Isotopes -

Atoms of an element that have the same number of protons but different numbers of neutrons

Question 15

●The only real difference between two isotopes of the same atom is their…

Answer 15

Mass

Question 16

Atomic Mass-

Answer 16

Atomic Mass-
The average mass of all the atom’s isotopes
●This is the decimal number on the periodic table
●Unit is amu (atomic mass unit)

Question 17

Heisenberg university principle

Answer 17

We cannot know the position and the speed of a moving object simultaneously

Question 18

Principal energy levels

Answer 18

N=1, n=2, n=3, n=4, etc

Question 19

Which energy level is the lowest of energies and is the easiest for electrons to live in?

Answer 19

1st energy level

Question 20

The number of sub levels is…

Answer 20

Equal to the value of n

Question 21

2nd sub level

Answer 21

(N=2) has 2 sub levels, 2s and 2p

Question 22

Order of letter sub levels

Answer 22

S,p,d,f

Question 23

Construction of an atom

Answer 23

Principal of energy level-sublevel-orbital-electron

Question 24

S Sublevels

Answer 24

1 orbital

Question 25

P sublevels

Answer 25

3 orbitals

Question 26

D sublevels

Answer 26

5 orbitals

Question 27

F sublevels

Answer 27

7 orbitals

Question 28

Max number of electrons on each orbital

Answer 28

2

Question 29

Sphere

Answer 29

1 type

Question 30

Dumbbell

Answer 30

3 types

Question 31

Complex

Answer 31

5 types

Question 32

Very complex

Answer 32

7 times

Question 33

Electron configuration

Answer 33

Distributions of electrons among the orbitals of an atom

Question 34

How electron configuration determined

Answer 34

By distributing the atom's electrons among ---levels - --sublevels - --orbitals

Question 35

Ground state

Answer 35

Electrons occupy lowest energy orbitals available to the most stable lowest energy state of an atom (this is how electrons normally exist)

Question 36

Aufbau principle

Answer 36

Electrons added 1 at a time to lowest energy orbital available

Question 37

Pauli exclusion principle

Answer 37

An orbital can hold a maximum of 2 electrons and they must have opposite spins

Question 38

Hund's rule

Answer 38

Electrons will occupy equal energy orbitals so that a max number of unpaired electrons results

Question 39

Orbital diagram

Answer 39

Shows the location of the electrons according to 3 principles

Question 40

How to write an electron configuration

Answer 40

Determine the # of electrons in an atom or ion, then using the arrows chart, place the electrons in the lowest energy's sub levels

Question 41

Democritus

Answer 41

450 BC Proposed the idea that matter was not infinitely divisible

Question 42

Lavoisier

Answer 42

1700s law of conservation of matter

Question 43

Proust 1700s

Answer 43

Law of definite proportions

Question 44

Dalton

Answer 44

1803 Dalton's Atomic Theory