Science (atoms)

Question 1

Define the term matter

Answer 1

Anything that has mass and takes up space

Question 2

Define the term Atom

Answer 2

The smallest part of an element that can exist

Question 3

Define the term element

Answer 3

a pure substance one type of atom, all look the same (they have the same number of protons and electrons)

Question 4

number of protons

Answer 4

The number of protons determines which element we have always the same

Question 5

What are electrons

Answer 5

Electrons are found on the outside of the atom

Question 6

symbol for proton

Answer 6

Pt proton - positive

Question 7

neutrons

Answer 7

N Neutron- neutral

Question 8

Electron symbol

Answer 8

E-

Question 9

what do protons and neutrons contribute to

Answer 9

to an atoms mass

Question 10

What mass do neutrons have

Answer 10

carry no change, they also have a mass of 1 amu

Question 11

What change does an electron have and mass and weight

Answer 11

negative change, they have no mass and weigh nothing

Question 12

protons and electrons have the same mass true or false

Answer 12

true

Question 13

Hydrogen symbol

Answer 13

H

Question 14

How many electrons can the first shell hop up to

Answer 14

2 electrons

Question 15

how many electrons can the second shell hold up to

Answer 15

8 electrons

Question 16

What are the first 12 periods on the table

Answer 16

hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, neon, sodium, magnesium

Question 17

what is the max for the third shell

Answer 17

8

Question 18

what is group 1 called

Answer 18

Alkali METALS

Question 19

what is group 2 called

Answer 19

ALKALEME EARTH METALS

Question 20

WHAT IS GROUP 7

Answer 20

HALOGENS

Question 21

WHAT IS GROUP 8

Answer 21

NOBLE GASES

Question 22

WHO WAS DIMITRI MENDELEEV

Answer 22

• THE FATHER OF THE PERIODIC TABLE
• HE GROUPED THE ELEMENTS BASED ON THEIR PROPERTIES

Question 23

The words atom, molecule and lattice refer……..

Answer 23

to how the atoms are connected

Question 24

Ionic compounds

Answer 24

• occurs when atoms loss or gain electrons
• These results in atoms that have a positive or negative charge and are called ions

Question 25

covalent compounds

Answer 25

- takes between non- metals - occurs when 2 or more atoms share electrons to achieve a full outer shell

Question 26

Where does energy transfer to?

Answer 26

Energy is transferred from the surroundings to the system to break the chemical bonds in the reactants

Question 27

Exothermic reactions

Answer 27

the exit of energy transfer from the system to the surrounding meaning more energy is released than is taken

Question 28

Endothermic reactions

Answer 28

The energy entering the system from the surroundings cause the temp of the surroundings to decrease meaning more energy is taken in than is released when new bonds are made

Question 29

symbol for Fluorine

Answer 29

F

Question 30

SYMBOL FOR SILICON

Answer 30

Si

Question 31

symbol for sodium

Answer 31

Na

Question 32

Who was john Dalton

Answer 32

- Drew upon the ancient Greek idea of atoms -solid sphere model - His theory stated that atoms are indivisible (when they were subatomic particles) - compounds are a combination of different types of atoms

Question 33

Who was J.J Thompson

Answer 33

- plum pudding model - discovered electrons in 1897 (won a noble prize - it shows the atom as composed as electrons scattered throughout a spherical cloud positive charge - recognised electrons as components of atoms

Question 34

who was Ernest Rutherford

Answer 34

- Physicist, known as the "father of nuclear physics." - Discovered the structure of the atom, including the nucleus. - Gold Foil Experiment: Conducted the famous experiment in 1909, which led to the discovery of the atomic nucleus. -Theory: Proposed the planetary model of the atom, where electrons orbit a dense, positively charged nucleus. His work laid the foundation for modern atomic physics and nuclear energy.

Question 35

who was Niel Bohr

Answer 35

- modified Rutherford's model of the atom by stating that electrons oved around the in orbits of fixed sizes and energies - planetary model - electrons could not occupy values of energy between the fixed energy levels