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Question 1

Atom Definition

Answer 1

Smallest Part Of An Element That Can Exist

Question 2

Molecule

Answer 2

Cluster Of Non-Metal Atoms Chemically Bonded Together

Question 3

Element

Answer 3

Substance That Contains One Type Of Atom

Question 4

Compound

Answer 4

Two Or More Elements Chemically Combined In Fixed Proportions.

Question 5

Who first proposed the idea that the atom wa sthe smallest thing?

Answer 5

Democritus

Question 6

What did Dalton’s evidence support?

Answer 6

The idea that atoms existed.
They were tiny spheres that couldn’t be divided.

Question 7

What did JJ Thompson discover and when?

Answer 7

In 1897, he discovered that atoms are made up of smaller particles.
He then made his plum pudding model.

Question 8

What was the Geiger-Marsden-Rutherford experiment?

Answer 8

Fired alpha particles (large positively charged particles) at very thin gold foil.

Question 9

What were the results of the Geiger-Marsden-Rutherford experiment and what did they inidcate?

Answer 9

Most of the alpha particles went straight through the gold particles - Atoms are mainly empty space.
Some of the alpha particles were deflected - Center of an atom must have a positive charge.
Some of the alpha particles bounced straight back - Center of an atom must contain a great deal of mass.

Question 10

What did Bohr propose and when?

Answer 10

In 1913, Electrons orbit the nucleus in fixed shells or orbitals located at set distances from the nucleus.

Question 11

What did Chadwick prove and when?

Answer 11

Proved the existence of neutral particles called neutrons. 1932.

Question 12

What are the relative masses of the subatomic particles?

Answer 12

Electrons - Negligible
Protons - 1
Neutrons - 1

Question 13

What is the Atomic Number?

Answer 13

The number of Protons.

Question 14

What is the Mass Number?

Answer 14

Number of Protons + Number of Neutrons

Question 15

What determines what type of atom one is?

Answer 15

The number of protons.

Question 16

What is the name of the outermost shell?

Answer 16

Valence Shell

Question 17

What does the cell become if the outer shell is full?

Answer 17

Much more stable

Question 18

What is the rough radius of an atom?

Answer 18

1 x 10^-10 meters

Question 19

What are Ions?

Answer 19

Particles with a different number of protons and electrons so are electrically charged.

Question 20

Rough size of an atom’s nucleus in relation to the atom?

Answer 20

Less than 1/10,000 of the atom

Question 21

What are Isotopes?

Answer 21

Atoms of the same element with different numbers of neutrons and the same number of protons.

Question 22

Why do isotopes of the same element have the same characteristics and chemical properties?

Answer 22

Because they have the same number of electrons in their outer shell.

Question 23

Calculating the relative mass of an atom.

Answer 23

(% of Isotope a x Mass of Isotope a) +
(% of Isotope a x Mass of Isotope a)
/
100

Question 24

What is relative atomic mass equal to?

Answer 24

1/12 of the mass of a Carbon-12 atom.

Question 25

What do Ions have the same stable electron structure as?

Answer 25

Noble Gases

Question 26

Which elements react to form posistive ions?

Answer 26

Metals

Question 27

What did the Plum Pudding Model suggest?

Answer 27

The atom is a ball of positive charge with negative electrons embedded in it.

Question 28

Where is the majority of an atom's mass found?

Answer 28

Its nucleus

Question 29

How can compounds be separated?

Answer 29

Chemical Reactions

Question 30

Group 1

Answer 30

Alkaline Metals

Question 31

Group 7

Answer 31

Halogens

Question 32

Group 0

Answer 32

Noble Gases

Question 33

Examples of Physical Change:

Answer 33

No new substance produced. Inolves the forces of attraction between particles. Examples include: melting point, boiling point, density, conductivity.

Question 34

Examples of Chemical Change:

Answer 34

New substance produced. Involves the transfer/sharing of electrons. Examples include: reactions with oxygen and water.

Question 35

How many electrons are in the valence shells of an Alkali Metal?

Answer 35

1

Question 36

Before the discovery of subatomic oarticles, how did scientists classify elements?

Answer 36

In order of their atomic weights

Question 37

Who changed the classification of elements?

Answer 37

Mendeleev

Question 38

Elements that do not form positive ions

Answer 38

Non-Metals

Question 39

What happens to the boiling point of the Noble Gases as their relative mass increases?

Answer 39

Increases

Question 40

What happens to the reactivity of the Alkali Metals as you go down the group?

Answer 40

Increases

Question 41

Number of electrons in the valence shell of the Halogens?

Answer 41

7

Question 42

What do the Halogens consist of?

Answer 42

Molecules made of pairs of atoms.

Question 43

What happens when you go down the the Halogens group?

Answer 43

The relative molecular mass, boiling point and melting point increase. The reactivity decreases.

Question 44

What does a more reactive halogen do to a less reactive halogen in an aqueuous solution of its salt?

Answer 44

It displaces it

Question 45

Who began developing the idea of a periodic table 140 years ago?

Answer 45

John Newlands

Question 46

What to do for a Six Marker?

Answer 46

Do a labelled diagram of the atom, draw the electrons and add the neutrons and protons. Say the number of protons, neutrons and electrons. Say the group and period and the feasons why. Say the electron configuration.