Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry MYP > MAIN POINTS > Flashcards

MAIN POINTS Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Transformation of States of Matter

A

Deposition: Gas to Solid

Condensation: Gas to Liquid

Sublimation: Solid to Gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Mixtures

A

Suspensions: Heterogeneous mixture of solute and solvent where the solute particles do not get dissolved in the solvent
Ex. Mud Water

Colloids: Heterogeneous mixtures that scatter light but don’t settle out.
Ex. Milk

Emulsions: Two immiscible liquids
Ex. Paint

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

List 5 properties of Ionic compounds

A

High m.p. and b.p.
Brittle
Soluble in water
Good conductors of electricity (only in water form)
Can conduct heat (in solid and water form)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

List 4 properties of (covalent) molecular bonding

A

Bad conductor of electricity
Low m.p. and b.p.
Do not dissolve in water
Dissolve in organic solvent (ethanol)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Bonding

A

non-metal +non metal –> Covalent

metal + non metal –> Ionic

metal + metal –> Metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Isotopes

A

Same number of protons different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Protons/ Neutrons/ Electrons in an element

A

Protons: Equal to Atomic Number

Neutrons: Atomic mass- Atomic Number

Electrons: Equal to Atomic Number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

To calculate rate of reaction

A

Amount of mass lost/ time or amount of product formed/time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Properties of Group 1 and Group 2

A

Group 1: Alkali Metals
-Highly Reactive
-Low m.p. & b.p.

Group 2: Alkaline Earth Metals
-Less reactive compared to alkali but still very reactive
- Higher m.p. & b.p. than alkali metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Properties of Group 7

A

Halogens
-Highly reactive
-Non metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Properties of Group 18

A

Noble Gases
-Inert reactivity
-Very low b.p. and m.p

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Properties of Group 5

A

Transition Metals
-High m.p. & b.p.
-Act as catalyst in reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Specific heat capacity

A

The amount of energy required to increase the temperature of 1kg of a substance by 1 degrees C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Endo/ Exo

A

Endothermic: Heat absorbed during reaction (-Delta H)

Exothermic: Heat released during reaction (+Delta H)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

How to calculate Delta H

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

List 7 properties of Acids

A

Tastes sour
Turns blue litmus paper to red litmus paper
Reacts with metals to form hydrogen gas
Forms H+ Ions
pH less than 7
Neutralises bases
Good conductors of electricity

16
Q

List 5 properties of Bases

A

Slippery, bitter
Turns red litmus paper blue
Usually forms OH- Ions
Neutralises acids
pH is greater than 7

17
Q

Soluble Salts making

A

Acid+Base –> Salt + Water

Acid+Metal –> Salt + Hydrogen

Acid+Metal Carbonate –> Salt + Co2 + H20

18
Q

Tests for Hydrogen & CO2

A

Hydrogen: When a lighted splint is inserted, a pop sound is heard

CO2: When bubbled through Calcium Hydroxide, CaCO3 is formed.

19
Q

Example of Strong Base

A

NaOH (Sodium Hydroxide)
KOH (Potassium Hydroxide)

20
Q

Oxides

A

Basic: Form basic metal oxides which are generally ionic in bonding. React with acids to form salts

Neutral: No reaction with anything

Acidic Oxide: Non metals react with oxygen to make acidic oxides

Amphoteric Oxide: Metallic Oxides which react with acids and alkalis

21
Q

Indicator (4)

A

Universal Indicator:
More specific pH value (universal indicator colour chart)
Acid = Red
Neutral = Green
Base = Purple

Litmus:
Acid = Red
Alkali = Blue

Phenolphthalein Indicator:
Acid= Colourless
Neutral= Light Pink
Base= Dark pink
Used in strong base-weak acid titrations

Methyl Orange Indicator:
Acid= Red
Neutral= Yellow orange
Base= Yellow
Used in weak base-strong acid titrations

21
Q

Titration Experiment (Apparatus)

A

Burette and Pipette and Conical flask

22
Q

Le-Chatlier’s Principle

A

If we change the factors affecting equilibrium then the reaction will shift in the direction where the effect is minimised.

22
Q

Factors Affecting Equilibrium

A

Temperature: If you increase the temperature of an already existing exothermic reaction it will become an endothermic reaction.

Pressure: Increasing- Equilibrium will shift where number of gaseous particles are less

Concentration: If concentration of reactants/ if concentration of products is decreased, it will shit towards the forward direction.

Catalyst: To reach equilibrium faster

23
Q

Factors Affecting Haber Process

A

Temperature: Since the reaction is an exothermic reaction, we would need a lower temperature (450 degrees) to favour the forward reaction. However, to have a high rate of reaction we need a high temperature. 450 degrees is a compromise, low yield for high rate of reaction.

Pressure: We would need a high pressure as there are fewer molecules of product than there are reactants. We also need a high pressure for high rate of reaction

Pressure: 200atm

24
Q

Reduction/ Oxidation

A

Reduction:
Loss of Oxygen
Gain of Hydrogen
Gain of electrons
The substance (reactant) which reduces is the oxidizing agent/ oxidant

Oxidation:
Gain of Oxygen
Loss of Hydrogen
Loss of electrons
The substance which oxidizes is the reducing agent/ reductant

Reduction happens at cathode (Red-Cat)
Oxidation happens at anode (An-Ox)

24
Q

Electrorod/ Electrolyte

A

Electrod: Cathode and Anode
Cathode attracts cations (+)
Anode attracts anions (-)
Is a rod of metal or graphite through which an electric current flows into or out of an electrolyte.

Electrolyte: Is the ionic compound (liquid basically) in a molten or aqueous solution that conducts electricity

25
Q

Oxidation Rules (6)

A

Uncombined Element= 0
Simple Ions= Valency
Elements in compound= add to 0
Polyatomic Ions= Sum of elements = charge of ion
Hydrogen= +1
Oxygen= -2

26
Q

Function of salt bridge in voltaic cell

A

1) The salt bridge helps to maintain the neutrality of the solution.

2) Movement of ions (cation to cathode and anion to anode) takes place via the salt bridge.

Salt Bridge contains metal salts like KNO3

26
Q

Half equation of oxidation and reduction

A

Cu2+(aq) + Zn(s) –> Zn2+(aq)+ Cu(s)

Zn(s) –> Zn2+ + 2e- (oxidation half reaction)

Cu2+(aq) + 2e- –> Cu (reduction half reaction)

27
Q

Factors affecting voltaic cell

A

Electrode Material: Zinc- as the anode
Copper- as the cathode

Electrolyte Concentration: Increased ion concentration in the electrolyte enhances the rate of chemical reactions, leading to higher voltage

Temperature: Higher temperature leads to a lower voltage due to higher internal resistance

Surface Area of Electrodes: Larger surface area: Greater contact between electrodes and electrolyte, faster reactions, higher voltage.

Chemistry MYP (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions