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
What is the mass number?
Sum of protons and neutrons
26
What is atomic notation?
27
What is an ion?
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
What substance loses electrons to form a positively charged ion?
Metals
29
What substance gains electrons to form a negatively charged ion?
Non-metals
30
What is a molecular compound?
A compound that is made from 2 or more elements, sharing electrons generally, molecular compounds form between NON-METAL ELEMENTS
31
Are all molecular compounds molecules?
Yes, all molecular compounds are molecules, but not all molecules are molecular compounds.
32
Physical Properties of Covalent Compounds
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
What is the difference between Ionic and Molecular compounds?
Ionic compounds take away electrons to fill there valence shell Molecular compounds use covalent bonds to share electrons.
34
How do ionic compounds form
When a positive ion attracts a negative ion to form an ionic bond
35
Are all compounds molecules?
Yes, but not all molecules are compounds
36
Where are Akali Metals located?
Group 1
37
Where are alkaline earth metals?
Group 2
38
Where are Halogen Gases?
Group 17
39
Where are Noble gases?
Group 18
40
Within A period all elements have the same?
Energy Levels/Valence Shells
41
Within a group all elements have the same number of?
Valence Electrons
42
Reactivity of metal increases as?
energy level increases
43
Reactivty of non-metals increase as
energy levels decrease
44
Atomic radius increases a
the energy level increases from top to bottom
45
Reactivity of metal increases from
_right__ to _left___ or _top__ to _bottom__.
46
Reactivity of non-metals increase from
left to right or top to bottom
47
Atomic radius increases from
right to left or top to bottom
48
Rank the 4 types of elements on the periodic table from most reactive to least.
- alkali metals: highly reactive - halogens: highly reactive - alkali earth metals: reactive - noble gases: not reactive
49
a) ____ likes to lose electron(s) to achieve maximum stability. __-___ likes to gain electron(s) to achieve maximum stability.
Metals like to lose elctrions Non-metals gain electrons
50
Why are the Alkali Metals and Halogens so reactive?
- alkali metals only have one valence electron - halogens are only missing one valence electron