Section 1.1 Quiz

Question 1

What is Matter?

Answer 1

Matter is anything that takes up space and has mass.

Question 2

What is an atom?

Answer 2

An atom is the basic building block of all matter and chemistry. It is the smallest unit into which matter can be divided and still retain the characteristic properties of an element.

Question 3

What sub-atomic particles are in an atom?

Answer 3

It is composed of three sub-atomic particles: the proton, the neutron, and the electron.

Question 4

John Dalton (1766-1844)

Answer 4

Dalton is the “Father of Atomic Theory”
Based on Dalton’s Atomic Theory, most scientists in the 1800s believed that the atom was like a tiny billiard ball that could not be broken up into parts (cap… Now we know that he is wrong)
All atoms of a given element are identical, having the same:
Size
Mass
Chemical properties
All atoms of different elements are different.

Question 5

JJ Thomson (1856-1940)

Answer 5

The Thomson model is usually called the plum pudding model.
He used cathode rays to prove that Dalton’s billiard ball model could be broken into smaller particles
Cathode rays are quite easy to produce, electrons orbit every atom and move from atom to atom as an electric current.
Thomson is credited with discovering electrons.

Question 6

Rutherford (1871-1937)

Answer 6

Rutherford’s model of the atom is sometimes called the planetary model.
The electrons orbit the nucleus like the planets revolve around the sun.
Used the Gold foil Experiment to discover the existence of:
An atomic nucleus’s
Protons

Question 7

Niels Bohr (1885-1962)

Answer 7

He experimented with light and its interactions with matter to develop a new model.
Disproved Rutherford’s Planetary Model
He showed that electrons can exist in specific energy levels.
His energy levels are called electron shells.
The electrons orbit the nucleus at fixed energy levels.

Question 8

Bohr’s Energy Level Model

Answer 8

Electrons are arranged in circles around the nucleus. Each circle has a different energy.
Electrons are in constant motion, travelling around the circles at the speed of light.
Electrons can “jump” from one circle to the next
But they can’t go in the nucleus, they travel too fast to be fully attracted

Question 9

Erwin Schrodinger (1887-1861)

Answer 9

This model is usually called the electron cloud model of the atom.
Schrodinger showed:
Electrons move in a region of space, often represented visually as a cloud.
Schrodinger wave equation, that describes the atom in terms of energy.
The solution to the equation shows that elections do not travel in precise orbits but instead exist in defined regions of space.

Question 10

What is a Nucleus?

Answer 10

posses’ protons and neutrons surrounded by a “cloud” of electrons.

Question 11

Atomic number

Answer 11

(Z)
number of protons/ electrons in a neutral atom

Question 12

Mass number

Answer 12

(A)
the sum of protons and neutrons in the nucleus
Example: Carbon = 6 protons/ 6 neutrons/ 6 electrons
Z = 6, A = 12

Question 13

Electron mass aprox? (kg)

Answer 13

9.11x10^-31

Question 14

Protons mass aprox? (kg)

Answer 14

1.67x10^-27

Question 15

Neutron mass aprox? (kg)

Answer 15

1.67x10^-27

Question 16

How do you find the # of neutrons in an atom?

Answer 16

The number of protons plus the number of neutrons is equal to the mass number.
Therefore,

Total neutrons = mass number - atomic number.

Question 17

How do you find the # of electrons in an atom?

Answer 17

When the atom is neutral, equals the number of protons

Question 18

How do you find the # of protons in an atom?

Answer 18

The atomic number

Question 19

What is the signifigance of Carbon?

Answer 19

Carbon is taken as a reference because it is the same in all places.
Carbon is so abundant and it makes the average very precise.

Question 20

Lewis Diagram

Answer 20

Lewis diagram is a model of an atom that has the chemical symbol for the element surrounded by dots to represent the valence electrons.
Also called the electron dot diagram
It is only useful if the atom has 8 or fewer electrons in the outer shell. (columns 1,2 and 13-18)
Only Valance electrons are shown in the Lewis diagram.

Question 21

What is a valence electron?

Answer 21

Valance electrons are these in the outer shell and are the only electrons involved in bonding.

Question 22

what is the formula for the amount of electrons that can ocupy a shell?

Answer 22

The maximum number of electrons that can occupy a shell can be calculated by using the formula 2n²

Question 23

max for shell 1

Answer 23

2*1² = 2

Question 24

max for shell 2

Answer 24

2*2² = 8

Question 25

max for shell 3

Answer 25

2*3² = 18

Question 26

max for shell 4

Answer 26

2*4² = 32

Question 27

max for shell 5

Answer 27

2*5² = 50

Question 28

max for shell 6

Answer 28

2*6² = 72

Question 29

Isotopes, what are they?

Answer 29

Atoms of an element with the same atomic number but different mass number
The difference is in the number of neutrons

Question 30

Radio Isotopes, What is this yes yes?

Answer 30

Radiation is released when the atoms of one isotope are transformed into atoms of a different isotope
This occurs because the nucleus is unstable, I.e., The neutrons and protons are not properly balanced so the nucleus decays into a more stable nucleus, I.e, a Radio Isotope.
A neutron decays into an electrons and a proton so the nucleus now has one more proton and one less neutron. The electron is ejected as a beta particle.

Question 31

An isotope is named in two ways:

Answer 31

The mass number attached to the atom name. Itst this one way?????? oh well…

Question 32

what is the special name for Hydrogen-1?

Answer 32

Protium

Question 33

what is the special name for Hydrogen-2?

Answer 33

Deuterium

Question 34

what is the special name for Hydrogen-3?

Answer 34

Tritium