Chemistry Chapter 3 10.15.05

Front 1

Atom

Back 1

The smallest particle of an element that retains the chemical properties of that element

Front 2

Electron Cloud

Back 2

Region that is occupied by electrons

Front 3

Proton

Back 3

Are P+ and are positive

Front 4

Nuclear Forces

Back 4

Short range proton-neutron, proton-proton, nuetron forces hold the nuclear particle together

Front 5

Electron

Back 5

Are E- and are negative

Front 6

Neutron

Back 6

Are N and neutral

Front 7

Thomson

Back 7

Revealed that the electron has a negative charge using the plum pudding experiment

Front 8

Rutherford

Back 8

Led in the gold foil experiment

Front 9

Millikan

Back 9

Determined that electrons have a negative charge using the oil drop experiment

Front 10

Democritus

Back 10

Had the earliest particle theory of matter in 400 bc. He called it a atom and said it was indivisible

Front 11

Dalton

Back 11

Created the atomic theory in 1808 where he came up with five ideas on atoms

Front 12

Law of Conservation of Mass

Back 12

Mass is neither destroyed nor created during ordinary chemical reactions or physical changes

Front 13

Law of Multiple Proportions

Back 13

If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

Front 14

Law of Definite Proportions

Back 14

The fact that a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound

Front 15

Isotopes

Back 15

Atoms of the same element that have different masses

Front 16

Average Atomic Mass

Back 16

The weighted average of the atomic masses of the naturally occurring istopes of an element

Front 17

Nuclide

Back 17

General term for any isotope of any element

Front 18

Atomic Mass Unit

Back 18

Unit of mass that is exactly 1/12 the mass of a carbon-12 atom or 1.660

Front 19

Avogadros Number

Back 19

Number of particles in exactly one mole of a pure substance

6.02 x 10 23

Front 20

Mole

Back 20

Amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12

Front 21

Describe the gold foil experiment of Rutherford, Geiger and Marden. When did this happen?

Back 21

(1911) Bombarded a thin piece of gold foil with a narrow beam of alpha particles. Some of the particles were redirected by the gold foil back toward their source

Front 22

What was Rutherford's explanation. When did this happen?

Back 22

(1913) There is a small densely packed, postive nucleus. Electrons travel in a circular orbit around the nucleus

Front 23

What's in the nucleus and what are their charges

Back 23

Protons - Positive

Nuetrons - Nuetral

Front 24

Atomic Number (symbol)

Back 24

(Z) Is the number of protons in the nucleus of each atom of that element

Front 25

What element has the most stable isotope? How many does it have

Back 25

Tin

10 isotopes

Front 26

What are two ways you identify isotopes by

Back 26

1. The mass number is written with a hyphen after the name of the element

2. Show the composition of nucleaus

Front 27

Which particles determine the element

Back 27

Protons

Front 28

What are the three mass numbers of the 3 isotopes of hydrogen

Back 28

1, 2 and 3

Front 29

Mass Numbers (symbol)

Back 29

(A) Total number of protons and neutrons in the nucleus of an isotope

Front 30

How do the masses of the atomic particles compare

Back 30

Neutrons are slighty more massive than protons

Front 31

Atoms of different elements have _______ number of protons

Atoms of the same element all have the _________ number of protons

Back 31

Different

Same

Front 32

What parts of Daltons theory are not correct

Back 32

Atoms can be divisible into even smaller particles

Elements can have atoms with different masses

Front 33

State 5 points of Dalton's Atomic Theory. Whats the date of this theory

Back 33

(1808)
1. All matter is composed of atoms

2. Atoms of a element have the same size, mass, Atoms of different elements differ in size, mass etc.

3. Atoms cannot be subdivided, created and destroyed

4. Atoms of a different elements combine in simple whole number ratios to form chemical compounds

5. In chemical reactions atoms are combined, seperated, rearranged

Front 34

Earliest particle theory of matter was discovered by _________ in __________

He called this particle _________

Back 34

Democritus

400 b.c.

Atom

Front 35

Molar Mass (unit)

Back 35

The mass of a pure substance

g/mol

Front 36

How do you define the radius of an atom

Back 36

Distance from the center of the nucleus to the outer portion of this electron cloud

Front 37

When was it revealed that the electron has a negative charge

Back 37

1897