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MOD 1 Chem Year 11 > Module 1: Chapter 1 > Flashcards

Module 1: Chapter 1 Flashcards

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1
Q

Homogeneous

A

Uniformly mixed and the composition is uniform.
(e.g. sugar solution, filtered air

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2
Q

Heterogeneous

A

Components are not uniformly mixed

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3
Q

Centrifugation - meaning

A

Process where a mixture of solids in a liquid is separated through spinning the mixture at high speed in a horizontal plane.

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4
Q

Centrifugation - purpose

A

To separate solids of different particle size in an aqueous suspension

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5
Q

Centrifugation (steps)

A
  1. Suspension placed in a centrifuge tube
  2. The tube is then placed in a centrifuge
  3. Suspension is spun and heavy particles are rapidly separated from the lighter particles and are deposited at the end of the centrifuge tube.
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6
Q

Factors that influence centrifugation

A

Density of both samples and solution

Temperature / Viscosity

Distance of particle displacement

Rotation Speed

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7
Q

Porosity

A

Size and number of pores in a filter

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8
Q

Filtration

A

Used to separate solids that are suspended in liquids or solutions.

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9
Q

Miscible

A

Liquids that mix in all proportions to form one phase

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10
Q

Distillation

A

A common method of separating a mixture of miscible liquids.

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11
Q

What does distillation depend on?

A

Liquids components having significantly different boiling points.

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12
Q

What happens in distillation?

A

Vapour of the more volatile component is condense back to a liquid.

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13
Q

Distillate

A

Liquid which is condensed from a vapour during distillation.

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14
Q

Fractional Distillation

A
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15
Q

Magnetic Separation

A

When a magnet is used to separate substances which are attracted to metal from a mixture of substances that are not attracted to metal.

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16
Q

Gravimetric Analysis + why it is important

A

Analytical techniques used to measure the proportion of each component in a mixture

Allows analytical chemists to test products for composition and purity

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17
Q

Pure substances - types

A

2: elements and compounds

18
Q

Compounds - how they are separated, composition, types

A

Separated by chemical means

Composed of elements in fixed atomic ratios.

Classified as Inorganic and organic.

19
Q

Organic Compounds

A

Based on element carbon and produced by living organisms.

e.g. sugar, fats, proteins

20
Q

Inorganic compounds

A

Forms most of the non-living world, is composed of metals bonded to non-metals

21
Q

Naming rules for inorganic compounds

A

Metal named first
Non-metal named second
“Ide” suffix used for the non-metal in simple binary compounds.

22
Q

Properties of metals

A

lustrous when polished
good electrical conductors
good heat conductors
malleable
ductile

23
Q

Why are metals good electrical conductors?

A

Due to mobile(delocalised electrons)
–> electrons that are not bound to a particular atom but are free to move in a metal

24
Q

Which metal is not a solid?

A

Mercury - liquid at 25ºC

25
Q

Diatomic Molecules and states

A

H2, N2, O2, F2, Cl2, Br2, I2

First 5 are gases at room temp, Br is a liquid, and I is a solid

26
Q

Semi metals

A

Boron (B) , Silicon (Si) , Germanium(Ge), Arsenic (As), Antimony (Sb), and Tellurium (Te)

27
Q

Group 1 Properties and name

A

ALKALI METALS
Soft, highly reactive
Reacting with water produces strongly alkaline substances
High ph due to OH- ions
Reactivity increases down the group

28
Q

Group 2 Properties and name

A

ALKALINE EARTH METALS
Also produces alkaline solutions
Ocides, hydroxides, and carbonates are to as strongly alkaline as the equivalent Group 1 compounds
Reactivity increases down the group

29
Q

Group 17 Properties and name

A

HALOGENS
Can combine with metals to form salts
Fluorine is the most reactive of these halogens

30
Q

Group 18 Properties and name

A

NOBLE GASES
Unreactive elements under normal conditions

31
Q

Group 3-12 Properties and name

A

TRANSITION METALS
Less reactive than groups 1 and 2
Decreases down each transition metal group

32
Q

What is the atomic theory of matter and who proposed it?

A

John Dalton - 1802

All matter is made up of tiny spherical particles that are indivisible and indestructible

33
Q

Solution, Solvent, and Solute

A

Solution has one or more solutes DISSOLVED in a solvent

Solvent is a substance in which a solute dissolves

Solute is a substance that dissolves in a solvent

34
Q

What is the difference between aqueous and liquid solution?

A

Aqueous is when the water is a solvent whereas liquid is a pure substance in a melted state

35
Q

Suspension

A

Suspensions are heterogeneous, visually distinguishable parts, forms when substance does not dissolve significantly.
e.g. rbc in plasma

36
Q

Colloid

A

A mixture of particles that consists of smaller clusters of ions or molecules. Evenly dispersed throughout the solvent and do not settle on standing.

e.g. milk

37
Q

Properties of solids

A

Particles are close together

Strong attraction between particles

Vibrate in their positions

High Density

Extremely close particles held together in a fixed position

Cubic lattice

Incompressible and holds their shape

38
Q

Properties of Gases

A

Particles are far apart

Low density

Space to push particles closer together

Particles move in all directions

Compressible and take the shape of container

39
Q

Properties of Liquids

A

Particles are loosely packed

Fairly high

No space to push particles closer together

Yes particles can slide over each other, and change position

Liquids are incompressible and flow to adopt the shape of the container

40
Q

Ferrofluids

A

A liquid mixture that responds to magnetic fields.

When placed close to magnet it behaves like solid, and liquid far away from metal

MOD 1 Chem Year 11 (2 decks)

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