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Grade 10 Final Exam > Grade 10 Chem > Flashcards

Grade 10 Chem Flashcards

1
Q

How do you properly read the periodic table?

A

Columns = groups, periods = rows,
atomic number = # of protons top left
mass number = # of protons + neutrons bottom middle
Valence in top right corner
Symbol middle

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2
Q

Explain the bohr Rutherford model

A
  1. Shows electron shells and how many per shell. It’s used to explain all layers of an atom and is more time-consuming than other models to draw.
  2. shows neutrons and protons in the middle
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3
Q

Explain the lewis dot diagram

A
  1. Shows valence electrons only. It’s quicker to draw and is better than the Rutherford model is some cases.
  2. Element name in the middle
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4
Q

Explain isotopes

A
  1. The same # of protons and electrons but a different # of neutrons.
  2. Different atomic mass numbers (number of protons and neutrons in the nucleus)
    EX: Carbon-12 has 6 protons and 6 neutrons. While Carbon-13 has 6 protons and 7 neutrons.
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5
Q

Explain how to calculate the relative atomic mass

A

Relative Atomic Mass = sum of (isotope abundance x isotope mass #) / sum of isotope abundance.

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6
Q

What are the subatomic particles and their charges and weight

A

Proton: +1, 1
Electron: -1, 1/1837
Neutron: 0, 1

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7
Q

Explain the octet rule

A

For an atom to be stable they must have 8 valence electrons.

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8
Q

Explain ionic bonding

A
  1. Bonding between metal and non-metals.
  2. A transference of electrons turning the atoms into a cation and an anion to become stable.
  3. Held together by an electrostatic force of attraction. An example is a giant lattice structure.
  4. Ions are formed to become more stable than previously because they want to follow the octet rule.
  5. Ionic compounds can conduct electricity when dissolved in water due to the free electrons.
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9
Q

Explain covalent bonding

A
  1. Bonding between 2 non-metals
    Sharing of electrons
  2. They share to become more stable by following the octet rule.
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10
Q

Explain metallic bonding and its properties

A

Metallic Bonding: Bonding between 2 metals

  1. Before bonding, valence electrons are near their positive nucleus. After bonding, a sea of delocalized electrons surrounds the positively charged positive ions due to the loss of electrons and then forms a giant lattice structure.
  2. Can conduct electricity as the electrons are free.
  3. It’s malleable because the layers of metal ions can slide over one another.
  4. High BP and MP because of their strong lattice structure.
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11
Q

Explain naming conventions for ionic bonding

A
  1. Name cation then anion
  2. Cation retains same name
  3. Use root “ide” for anion
  4. For poly atomic ions, use the whole name
    EX: Magnesium Phosphide and Potassium carbonate
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12
Q

Explaiin naming conventions for covalent bonds

A

1) First element: Prefix with full element name. EX: Dinitrogen
2) Second element: prefix with root ending “ide” EX: fluoride
Exception: The prefix “mono” is not used with the first element in any case
Exception: Carbon almost always comes first
Exception: If the element ends with a vowel, then the prefix’s ending with an “a” or “o” is cut off.
All: Dinitrogen fluoride. Carbon dioxide not Monocarbon dioxide

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13
Q

State the chemical equations

A

5 types:
Synthesis: element A + element B = element AB
Decomposition: AB = element A + element B
Single displacement reaction: A + Bc = B + ac
Double displacement: AB + CD = AD +BC
Combustion: Fuel + o2 burns into h2o and co2

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14
Q

Explain combustion, its formula, how it reacts with non-metals/metals, and incomplete and complete combustion.

A

Combustion (exothermic reaction): The burning of fuels in the presence of oxygen.

Formula: Fuel + oxygen gas = products
(fuel has potential energy that can be released by heat)
Type 1: metals: when we burn metals, the oxygen and the metal bond together to create a solid metal compound and thus become heavier in the process.

Type 2: non-metals: when we burn non-metals, the oxygen, and the no-metals bond together to create gaseous products and diffuses thus creating a lighter product.

There are two types of combustion: complete which means that there is an excess of oxygen and incomplete meaning there is limited oxygen:

Type 1: Complete combustion produces carbon dioxide and water as gases.
Type 2: incomplete combustion produces either carbon monoxide and water or carbon as a solid and water.

the effects of the products: carbon dioxide contributes to global warming. Carbon monoxide is toxic.

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15
Q

Explain how to balance equations

A

By following the law of conservation of mass, we will add coefficients in front of the chemical molecules so that there are the same number of atoms on both sides of the equation.

Rule: We can’t add subscripts to an equation. Only coefficients

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16
Q

Explain how to calculate moles when given some of the following: c, n, and v.

A

Concentration: the amount of substance in a certain defined space or volume

n = number of moles
c = mol/dm3
v = dm3

Concentration calculations can be used to determine whether a solution is safe for experiments.

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17
Q

How do we calculate moles when given some of the following: N,n, and Na?

A

The variables represent:
N= number of particles
n= number of moles
Na= Avogadro’s constant which is 6.02 x 10^23

Substitute known information and solve accordingly.

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18
Q

Explain dilutions

A

Serial dilution: the mixing stock and solution to create a less concentrated version of the solution.

Method 1: Find the dilution factor
Divide the concentration of the stock by the concentration of the solution.
EX: You have an initial stock solution with a concentration of 2.0M and
need to make 20cm3 of a 0.4M solution. 2.0/0.4 m = 5

Because the solution will be 5 times more dilute, you will need to use 5 times less of it.
To find out how much stock solution to add, divide the total volume of the solution you
will make by the dilution factor.
volume of stock solution transferred = 20cm3 ÷ 5 = 4cm3
You will add 4cm3 of the stock solution, then dilute it with distilled water to get the total volume that you need. The total volume minus the transferred volume will give you the volume of distilled water you need to add.
distilled water added = 20cm3 – 4cm3 = 16cm3

Method 2: C1V1=C2V2

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19
Q

Explain fractional distillation/distillation.

A

Fractional distillation: a process that separates crude oil into different hydrocarbon chains. If the chain is short, then it has a low BP, and vice versa.

Distillation: the process used to separate ethanol and water

Different liquids are poured at the bottom. Vapours start at the hot bottom and rise as it gradually gets cooler. Vapors condense when they reach a column that is below their boiling point.

Long-chain hydrocarbons will condense at the bottom where it is the hottest.

Examples are: bitumen, petrol and diesal.

20
Q

Explain alkanes vs alkenes

A

Alkanes:
Formula: Cn = H2n+2
Alkanes are saturated
Meth, eth, prop, but, penta, hexa, hepta, oct, non, and dec
Alkenes:
Containing at least one carbon double bond
Formula: Cn=H2n
naming conventions are the same throughout alkanes, alkenes, and alcohols.

21
Q

Explain cracking

A

The separation of different hydrocarbons into smaller chain lengths of hydrocarbons.
Alkane -> Alkane + Alkene

If a alkene is unsaturated, it can still be broken up.

22
Q

What is Amu

A

AMU: defined as the mass of 1/12 of a carbon 12 atom. This mass unit is used when calculating relative atomic mass.

23
Q

Explain alloys and whether they’re better than pure metals.

A

Alloys are beneficial when: Attempting to make a stronger, less malleable, less ductile metal. For purposes such as knives or swords.

This is because by adding the extra atom particles, more space is taken inside the compound. Thus as a result making it more difficult for the layers to slide over one another and thus stronger.

24
Q

Explain how the products of combustion can be seen/proven/shown

A

The products can be teseted via colbalt chloride paper where the paper starts off blue and turns into a pink color due to the presence of water.

can be tested via limewater as limewater turns cloudy due to carbon dioxide.

25
Q

Explain the difference between relative atomic mass, relative molecular mass, and relative formula mass

A

Relative atomic mass: the average mass of all isotopes of a particular element
Relative molecular: the relative atomic mass of the atoms within a molecule
Relative formula: the relative atomic mass of atoms within a formula

26
Q

Explain the enhanced greenhouse gas effect.

A

Is the green house gas effect but is caused by human activity.

27
Q

Explain two environmental effects of combustion

A

Acid rain: any form of precipitation with acidity. Human causes: burning or combustion.

Greenhouse gas effect: Gases absorb heat from the sun and exacerbate global warming.

28
Q

Explain alcohols

A

A homologous series which contains the -OH group.

The naming is as follows: Meth,eth, prop,but, penta, hexa, hepta, oct, non, and dec.

General formula: CnH2n+1,OH

29
Q

Define the law of conservation of mass

A

Atoms can not be created nor destroyed but only combined

30
Q

What are the 3 forms of fossil fuels?

A

Natural gas, coal, and crude oil

31
Q

Explain why a short-chain hydrocarbon has a low BP and MP and a long-chain hydrocarbon has a high MP and BP

A

A longer chain hydrocarbon means that more kinetic energy is needed to pull them apart and thus condense.

32
Q

Define “Homologous Series”

A

A sequence of compounds with the same functional group and similar chemical properties. EX: A functional group could be like OH of alcohols.

33
Q

What does the term “Saturated” mean in Alkanes and Alkenes?

A

Saturated means that the compounds only contain SINGLE BONDS. Alkanes only contain single bonds therefore all alkanes are saturated.

34
Q

Outline the alkane/alkene naming conventions

A

The end depends on what type of homologous series it is.
The first part of the name follows a Greek naming system and is as follows.
Meth, Eth, Prop, But, Pent, Hex, Hep, Oct, Nona, and Deca.

35
Q

How can we determine whether a compound is an alkane or an alkene?

A

We can use bromine water. If the compound is an alkene: the double bond can be broken and bond with the compound and thus make the bromine water, Br2, turn clear from a brownish color.
If it’s an alkane, then the water will stay the brownish color.

36
Q

What’s an endothermic and exothermic reaction?

A

Endothermic reaction absorbs heat while exothermic releases heat.

37
Q

What’s the general formula for Alkane, Alkene, and alcohols?

A

Alkanes: Cn = H2n+2
Alkenes: Cn= H2n
Alcohols: Cn=H2+1

38
Q

What is a lattice structure?

A

An ionic compound made of alternating positive and negative ions which are equally attracted to the opposite ion around them (there are 6) by the electrostatic force of attraction of ionic bonds.
This is called a giant ionic lattice

39
Q

What are the 7 diatomic elements?

A

Iodine, bromine, chlorine, fluorine, oxygen, nitrogen, hydrogen
or
I bring cookies for our new home

40
Q

In ionic compounds when it shows Iron (II) chloride, what does the number mean?

A

The number represents the number of positive charges. So in this case, it has a +2 charge.

41
Q

How do we perform dilutions and for what purpose.

A

In dilutions:

Adding water or other solutions to a mixture to create a less harmful or acidic alternative. To calculate how much we need to add we use the formula C1V1=C2V2

C1= concentration of stock
V1= amount of stock transferred
C2= concentration to make
V2= total volume. (Have to add both volumes together)

42
Q

What are some real-life applications of isotopes?

A

Copper-67: a radioactive isotope used in radionuclide therapy.

43
Q

Explain how to calculate moles when given some of the following: g, moles, and g mol-1.

A

The variables represent:
g = mass
moles = amount of substance
g mol-1= molar mass

Substitute known information and solve accordingly.

44
Q

What is the fermentation of glucose and its advantages?

A

Glucose from plant materials is converted into ethanol and carbon dioxide by adding yeast.

Advantages: low cost, renewable

45
Q

What is the rehydration of ethanol and its advantages?

A

Ethene is heated with steam and turns it into ethanol.
Ad: uses crude oil, purer product, renewable source

Grade 10 Final Exam (3 decks)

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