Matter unit

Question 1

Define chemistry

Answer 1

The study the composition and properties of matter

Question 2

Define Matter

Answer 2

Any substance that has mass and has volume (occupies space)

Question 3

What is all matter composed of

Answer 3

Atoms

Question 4

Charge, atomic mass, and symbol of protons

Answer 4

+ charge , 1u atomic mass unit, p+

Question 5

Charge, atomic mass, and symbol of neutron

Answer 5

Neutral charge, 1u (atomic mass unit) , n0

Question 6

Charge, atomic mass, and symbol of electrons

Answer 6

Negative charge, 1/2000 u (atomic mass unit), n-

Question 7

Where are protons and neutrons contained

Answer 7

In the nucleus

Question 8

Where are electrons found

Answer 8

In orbit around the nucleus

Question 9

Define molecules

Answer 9

2 or more atoms bonded together
Hofbrincle can be the same element

Question 10

Define properties

Answer 10

Characteristics that help describe and identify matter

Question 11

Define Physical property

Answer 11

Can be observed without changing one kind of matter into something new. Ex Colour texture odours lustre

Question 12

Define Chemical property

Answer 12

Observed when one kind of matter is converted into a different kind of matter. Ex mg produced hydrogen gas in acid.

Question 13

Define qualitative

Answer 13

Can be described in words but cannot be measured or expressed with numbers

Question 14

Define quantitative

Answer 14

Can be measured and expressed with numbers

Question 15

Physical changes

Answer 15

Affect the physical appearance of matter,but not it’s composition. (Change in physical properties only)

Question 16

Chemical change

Answer 16

Changes that alter the composition of matter (change in both physical and chemical properties

Question 17

The 5 Clues for a chemical change

Answer 17

Colour change
Production of gas (bubbles)
Precipitate (solid) formation
Heat absorbed or released
Light produced

Question 18

Bohr Rutherford vs Louis dot

Answer 18

Bohr Rutherford shows all electrons and the protons and neutrons in the nucleus where as Louis dot diagram shows valence electrons

Question 19

The periodic law

Answer 19

The periodic law states that the properties of elements repeat in a pattern when they are arranged by atomic number

Question 20

Groups in the periodic table

Answer 20

Alkali metals
Alkaline earth metals
Halogens
Noble gases
Transition metals

Question 21

Properties of metals

Answer 21

Shiny
Solid (most)
Malleable
Ductile
High Conductive

Question 22

Properties of metalloids

Answer 22

Some shiny some not
Solids
Brittle
Not ductile
Semi conductor

Question 23

Non metals

Answer 23

Not shiny
Brittle
Mostly gases
Not ductile
Not conductive (insulators)

Question 24

Reactivity

Answer 24

How easily and quickly elements react(combine)

Question 25

Reactivity of metals

Answer 25

Reactivity of metals goes down as you go right across the periodic table

Question 26

reactivity of non metals

Answer 26

The reactivity of non metals increases going left (not including noble gases)

Question 27

Isotopes

Answer 27

Isotopes are atoms that have the same number of electrons and protons but a different number of neutrons (same atomic number different atomic mass)

Question 28

Radio isotopes

Answer 28

Isotopes with unstable nuclei that release high energy particles when they break apart

Question 29

Average atomic mass

Answer 29

Weighted average of the atom masses and abundance

Question 30

Atomic radius

Answer 30

The size of an atomic (measured from the nucleus to the outer edges of the cloud like outer edges of the atom)

Question 31

Atomic radius pattern and reason behind it

Answer 31

Atomic radius increases going down the periodic table as there are more energy shells that make the valence electrons further from the nucleus and lowers the effective charge of nucleus as it’s blocked by the other shells Atomic radius increases going right as the valence electrons are on the same energy level however the charge of the nucleus is higher which pulls the valence electrons closer

Question 32

Ionic compounds

Answer 32

Ionic compounds are formed between a non metal and a metal, when the metal transfers its valence electrons to the mon metal. This results in the positively charged metal ion (cation) and negatively charged non metal ion(anion), which are attracted and form a bond

Question 33

Covalent bonds

Answer 33

Are between non metals, and occurs when they share electrons to get a full shell

Question 34

Ionic compound properties

Answer 34

Solid at room temp Hard High melting and boiling points High solubility in water Conductive in water and as a liquid

Question 35

Covalent bonds properties

Answer 35

Can be solid liquid or gas at room temp Soft Low melting and boiling point Usually low solubility in water Not conductive

Question 36

Diatomic elements

Answer 36

Hydrogen Bromine Fluorine Chlorine Iodine Oxygen Nitrogen

Question 37

Covalent compound prefixes

Answer 37

Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

Question 38

Common names

Answer 38

H20 - water NH3 - ammonia CH4 menthane H2S hydrogen sulphide

Question 39

Polyatomic ions

Answer 39

Poly atom ions are treated as normal ions in a compound

Question 40

Key oxyions

Answer 40

No3-1 So4-2 Po4-3 Co3-2 Clo3 -1 Io3-1 Bro3-1

Question 41

OxyContin change in name

Answer 41

+1 oxygen - pernitrate NO4 -1 Keyoxyion - nitrate NO3 -1 - 1 oxygen - nitrite NO2 -1 -2 oxygen - hyponitrite NO -1

Question 42

Oxyacids

Answer 42

Oxyions change ate to ic It’s to ous