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Chemistry 10 Flashcards

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1
Q

Describing Chemical Reactions

A

Chemists use equations to describe chemical reactions. There are 2 types of equations - Word and Chemical. instead of using an equal sign, they use an arrow to show what products form from certain reactants.

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2
Q

Arrow means

A

produces

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3
Q

What is a word equation?

A

using words (chemical names) to describe reactants and expected products.

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4
Q

Word equation - Solve
When fluorine gas is put in contact with calcium metal, calcium fluoride is produced.

A

Fluorine gas + Calcium metal -> Calcium Fluoride powder

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5
Q

Chemical equations

A

uses chemical formulas to describe reactants and expected products.
- Always includes the state of each substance.
- Two types - Skeleton & Balanced

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6
Q

Skeleton equations

A

Translates the chemical name to formula. Exact same as a word equation, just with chemical names and the state in brackets.

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7
Q

Skeleton equation - Solve
copper (ll) sulfate solution + iron -> iron (ll) sulfate solution + copper metal

A

CuSO4 (aq) + Fe (s) -> Cu (s) + FeSO4
(States are on periodic table)

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8
Q

What are Diatomic Elements?

A

These are elements that naturally come in two’s when found alone. When put together with other elements, there is only one of them. These elements are:
-Oxygen (O2)
-Hydrogen (H2)
-Nitrogen (N2)
-Fluorine (F2)
-Chlorine (Cl2)
-Bromine (Br2)
-Iodine (I2)
All of them come as gases except Bromine (l)

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9
Q

What is the global harmonized system?

A

a universal system used globally to describe safe handling of chemicals - you could go to any country and symbols would be the same and mean the same thing.

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10
Q

What is a coefficient?

A

A number that goes in front of the compound to tell us how many of that particular compound there is. It becomes a multiplier and helps us balance equations.

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11
Q

Rules of coefficients

A
  • We can only add in front of a compound.
  • Cannot put a coefficient in the middle of a compound
  • Cannot change or add subscripts
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12
Q

What is a subscript?

A

The “downstairs” number that tells you how many of one particular element/ion is in the compound.

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13
Q

What is the law of conservation of mass?

A

in any chemical reaction, the total mass of reactants equals the total mass of products. This is because mass cannot be created nor destroyed. We use conservation of mass when we are balancing equations because of this.

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14
Q

Types of chemical reactions

A

-Synthesis
-Decomposition
-Single Displacement
-Double Displacement
-Combustion
–> You only need to know how to predict the last three

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15
Q

Synthesis

A

a reaction that two reactions combine to create one large or more complex product.

A + B -> AB

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16
Q

Decomposition

A

A reaction in which one large or complex compound breaks down into to or more smaller compounds.

AB -> A + B

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17
Q

Single Displacement

A

A single displacement reaction is a chemical reaction in which one element is replaced by another compound.

AB + C -> AC + B

*YOU CANNOT REPLACE A NON METAL (-) WITH A METAL (+) OR VISE VERSA.

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18
Q

Double Displacement

A

A reaction in which two ionic compounds exchange ionic partners (Metal and Non -Metal)

AB + CD -> CB + AD

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19
Q

Combustion

A

A reaction in which a substance burns or reacts quickly with oxygen

  1. Lots of O2
  2. Burns quickly
  3. Forms Oxides
  4. Releases energy.
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20
Q

Exothermic reaction

A

Have energy as a product
- vessel will get hot

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21
Q

Endothermic reaction

A

Have energy as a reactant
- vessel will get cold

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22
Q

Rules for predicting products in chemical reactions

A

Pay attention to charges
DO NOT carry subscripts to other side
always balance last

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23
Q

Predicting Combustion

A

if you have a hydrocarbon (C,H,) and oxygen (O2) on the left hand side, you will have a combustion reaction. The product will ALWAYS be H2O and CO2.

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24
Q

Predicting single replacement

A

A metal can ONLY REPLACE ANOTHER metal and vise versa.
Will Always look like a lone metal OR a non-metal and an ionic compound.
- A metal will replace the cation (first name)
- A non-metal will replace the anion (last name)
PAY ATTENTION TO CHARGES

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25
Predicting double displacement
The reactants will always be 2 ionic compounds (Metal and Non-metal/polyatomic ion) -The two cations switch places. PAY ATTENTION TO CHARGES
26
Rate of reaction
How fast or slow the reactants turn into a product. If it takes a long time, it has a low reaction rate, if it is fast, it has a high reaction rate.
27
Reaction rate and concentration
Higher concentration - the most atoms there are and the more likely they will bump into each other faster
28
Temperature and rate of reactions
heat makes the molecules move faster and more likely to bump into each other
29
Surface area and rate of reactions
Higher surface area, the most area available for the reactants in a reaction.\ ex - twigs vs wood starting a fire, the twigs give more SA and therefore will burn faster.
30
Addition of a catalyst and rate of reactions
A catalyst speeds up the the reaction process by acting as building blocks to force the atoms together rather than by just leaving it for them to bump into each other.
31
Acids
-Taste Sour -Conduct electricity -Reacts with metals -Turns blue litmus paper RED -Reacts with Carbonates -Neutralizes Bases Acids release hydrogen when dissolved - the chemical formula always has an H at the start and (aq). Ex- HF (aq) Two types of acids - Binary Acids and Oxy-Acids
32
Binary Acids
Contains two elements - HYDROGEN and a NON-METAL - The name begins with the prefix "hydro" and ends in "acid" - The name of the non-metal has the ending changed to "-ic" Ex. HF (aq) = Hydrofluoric acid.
33
Oxy Acids
- Contain a polyatomic ion (That contains oxygen) and a Hydrogen Ion at the start. - Naming is the polyatomic ion ending in "-ic" followed by acid. Ex. HC2H3O2 (aq) = Acetic acid.
34
Bases
- Taste bitter - Feel slippery - Conduct electricity -turns red litmus paper BLUE -reacts with natural products (food, meats) eg. breaks down proteins.
35
Chemical formulas and bases
Most bases are ionic compounds that release hydroxide (OH) ions when dissolved. Chemical formula typically ends in OH and (aq), but compounds containing a carbonate (CO3, etc) at the end are also considered bases because they NEUTRALIZE ACIDS. Ex. NaOH (aq) - Sodium hydroxide NaHCO (aq) - Sodium Bicarbonate - Baking Soda
36
Colour with Acids & Bases
Acids and bases can cause chemicals to change colour. A substance that changes colour depending on acidity or basicity of the solution is called an acid-base indicator. ex. Bromothymol blue - Acid = yellow, base = blue Phenolphthalein - Acid = clear, base = pink Red litmus - acid = red, base = blue blue litmus - acid = red, base =blue.
37
pH scale
0-14 0-6 = Acid 8-14 = Base pH is a scale used to measure acidity or basicity in different substances. pH means power of hydrogen -> measures concentration of H+ ions. 1 unit on the scale is 10x. pH 3 is 10x more acidic than 4 pH 3 is 100x more acidic than 5 *decimals are okay (6.8 is still considered neutral, etc.)
38
pH scale - strong acids
battery acid stomach acid lemon juice
39
pH scale - strong bases
Liquid drain cleaner NaOH soapy water
40
pH scale - weak acids
unpolluted rain water tomatoes vinegar
41
pH scale - weak bases
baking soda ammonia windex
42
pH scale - neutral
Milk pure water egg whites
43
pH scale and soil
if it rains acid rain, certain crops need a more neutral base to survive. Acid rain can harm crops, so adding lime (a base), neutralizes the soil for them to thrive.
44
pH scale and shampoo/soap
Acidic shampoo restores hair flexibility and shine and is better when it comes to soaps. Basic soap (high pH) can damage skin cells, giving the appearance after the first wash of healthier skin, but really just stripping away layers of skin that protect us from infections.
45
Neutralization
This occurs when you mix an acid and a base together. Since they are opposites in many ways, by mixing them together, you are neutralizing them. Every single time that you do this, you will end up with water (H2O/HOH) + a certain type of "salt." The general structure of this is a double replacement. After this, the pH will become much closer to 7.
46
Ionic Compounds
These form when a metal and a non-metal/polyatomic ion combine. The atoms from the metal are transferred to the non-metal, combining them together.
47
Types of ionic compounds
Binary polyatomic
48
Molecular compounds
These form when two non-metals combine. The electrons are shared between the two non-metals.
49
Ways for molecular compounds to bond
1. single bond (1 electrons from each) 2. double bond (2 electrons from each) 3. triple bond (3 electrons from each)
50
Naming two non metals
ALWAYS END WITH IDE prefixes
51
Naming a metal and non-metal/ion
BALANCE CHARGES USING SUBSCRIPTS end in ide
52
Naming binary acids (non-metal)
always starts with hydro the end of the non-metal ends in ic end phrase with acid
53
Chemically formulating binary acids (non-metals)
Ex. hydrofluoric acid keep the H at the front for hydrogen keep the F in the middle end with (aq) HF (aq) DON'T FORGET TO BALANCE
54
Naming Oxyacids (polyatomic ions)
Keep the original name the same, but end with ic. Put acid on the end.
55
Chemically formulating Oxyacids (polyatomic ions)
Ex. Nitric Acid. Put H at the front for hydrogen, then the formula for your ion, then (aq) HNO3. DON'T FORGET TO BALANCE.
56
Recognizing ionic compounds
Metal at the start and non-metal at the end Or metal at the start and polyatomic ion at the end
57
Recognizing molecular compounds
if the words have prefixes Or if the chemical formula has two non-metals
58
Recognizing acids
H at the front of a non-metal or polyatomic ion with (aq) Or if the words have hydro and/or end in ic + acid.
59
Recognizing bases
metal at the front and OH OR CO3 at the end as well as (aq) Or if the words end in ide.
60
What will you get on this test?
100%
61
Endothermic
Heat as a reactant (ENter)
62
Exothermic
Heat as a product (EXit)
63
Strong acid example
HCl
64
Strong base example
NaOH
65
Weak acid example
H2C2H3O2
66
Weak base example
NaHCO3
67
what does (aq) stand for and what does it mean?
aqueous. It means it has been dissolved in water.
68

SCIENCE (9 decks)

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