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science gr.9 > Chem Exam review > Flashcards

Chem Exam review Flashcards

1
Q

What is a mechanical mixture?

A

Heterogenous=mixture of particles with more than one phase (different substances are visible)

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2
Q

What is a homegenous mixture?

A

Homogeneous=a mixture of particles with only one phase (different substances arent visible)

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3
Q

What is a compound

A

A compound is 2 or more elements in a fixed ratio

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4
Q

What is an element?

A

An element is 1 type of atom

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5
Q

What is a pure substance?

A

A pure substance is made up of only 1 type of particle

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6
Q

What is an atom?

A

A single neutral particle

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7
Q

List all quantitative physical properties:

A

melting point, boiling point, solubility, hardness, electrical conductivity,

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8
Q

List all qualitative physical properties:

A

flexibility, ductility, viscosity, luster,texture, mallebility, tastecolour, clarity, state, odour

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9
Q

List all the chemical properties of matter: Property Definition (Meaning)

A
  1. Combustibility Substance react with oxygen
  2. Reactivity
    w/water
    Substance reacting w/ water
  3. toxicity Substances causing harmful affects
  4. stability Ability of substance to remain unchanged
  5. Reactivity w/ air,
    acids, other pure
    substances
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10
Q

Define Physical Change

A

Change in substance that does not result in new substance

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11
Q

Define Chemical Change

A

Change in the composition of a substance

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12
Q

State three examples of physical change

A

Solubility
Change in shape/form
Change in state

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13
Q

State five clues/evidence of chemical change:

A

precipitate formed in liquid material New odor or gas bubbles forming
Heat or light produced or absorbed
Hard to reverse
A new colour that hasn’t been there before, formed

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14
Q

How do you calculate volume?

A

M/D

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15
Q

How do you calculate mass?

A

VxD

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16
Q

How do you calculate density?

A

M/V

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17
Q

Where is a proton, and what is it’s charge?

A

The proton is in in the nucleus and has a positive charge

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18
Q

Where is a neutron and what is it’s charge?

A

The neutron is also in the nucleus and has neutral charge

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19
Q

Where is an electron, and what is it’s charge?

A

An electron has negative charge and has a negative charge

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20
Q

State at least three physical properties of metals

A

Metals
-solid
-shiny
-good conductor
- high malleability
-high ductility

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21
Q

State at least three properties of non-metals

A

non-metals
-Mostly gas
-not shiny
-poor conductor
-low malleability
-low ductility

22
Q

State at least 3 properties of ionic compounds

A

High Melting Point and boiling Point
Electrical conductivity: Ionic compounds conduct electricity when dissolved in water or
Form crystal strucutures

23
Q

What is an ionic compound?

A

Ionic compounds are compounds made up of ions that form charged particles when an atom (or group of atoms) gains or loses electrons.

24
Q

What is the atomic number?

A

The number of protons in an element

25
Q

What is the mass number?

A

Sum of protons and neutrons

26
Q

What is atomic notation?

A
27
Q

What is an ion?

A

An ion is a charged atom which has an overall charge—either positive or negative—because the number of protons is different from the number of electrons.

28
Q

What substance loses electrons to form a positively charged ion?

A

Metals

29
Q

What substance gains electrons to form a negatively charged ion?

A

Non-metals

30
Q

What is a molecular compound?

A

A compound that is made from 2 or more elements, sharing electrons generally, molecular compounds form between NON-METAL ELEMENTS

31
Q

Are all molecular compounds molecules?

A

Yes, all molecular compounds are molecules, but not all molecules are molecular compounds.

32
Q

Physical Properties of Covalent Compounds

A

Strong attraction between atom, weak attraction between molecules, meaning low melting and boiling point

Solubility
Most covalent compounds are not soluble in water

Conductivity
Not conductive

33
Q

What is the difference between Ionic and Molecular compounds?

A

Ionic compounds take away electrons to fill there valence shell

Molecular compounds use covalent bonds to share electrons.

34
Q

How do ionic compounds form

A

When a positive ion attracts a negative ion to form an ionic bond

35
Q

Are all compounds molecules?

A

Yes, but not all molecules are compounds

36
Q

Where are Akali Metals located?

A

Group 1

37
Q

Where are alkaline earth metals?

A

Group 2

38
Q

Where are Halogen Gases?

A

Group 17

39
Q

Where are Noble gases?

A

Group 18

40
Q

Within A period all elements have the same?

A

Energy Levels/Valence Shells

41
Q

Within a group all elements have the same number of?

A

Valence Electrons

42
Q

Reactivity of metal increases as?

A

energy level increases

43
Q

Reactivty of non-metals increase as

A

energy levels decrease

44
Q

Atomic radius increases a

A

the energy level increases from top to bottom

45
Q

Reactivity of metal increases from

A

_right__ to _left___ or _top__ to _bottom__.

46
Q

Reactivity of non-metals increase from

A

left to right or top to bottom

47
Q

Atomic radius increases from

A

right to left or top to bottom

48
Q

Rank the 4 types of elements on the periodic table from most reactive to least.

A
  • alkali metals: highly reactive
  • halogens: highly reactive
  • alkali earth metals: reactive
  • noble gases: not reactive
49
Q

a) ____ likes to lose electron(s) to achieve maximum stability. __-___ likes to
gain electron(s) to achieve maximum stability.

A

Metals like to lose elctrions

Non-metals gain electrons

50
Q

Why are the Alkali Metals and Halogens so reactive?

A
  • alkali metals only have one valence electron
  • halogens are only missing one valence electron

science gr.9 (6 decks)

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