Matter and Chemical Change Flashcards
1
Q
Name the three danger symbols along with their shape and colour
A
Caution: Yellow, upside down triangle
Warning: Orange, diamond
Danger: Red, octagon
2
Q
Name the WHMIS symbols
A
Compressed gas, dangerously reactive material, oxidizing material, flammable and combustile material, biohazardous infectious material, corrosive material, poisonous and infectious causing other toxic effects/immediate and serious toxic effects
3
Q
Gas WHMIS symbol
A
Compressed gas
4
Q
“R” WHMIS symbol with a test tube
A
Dangerously reactive material
5
Q
“O” with fire flames WHMIS symbol
A
Oxidizing material
6
Q
Skull WHMIS symbol
A
Poisonous and infectious causing immediate and serious toxic effects
7
Q
Flames WHMIS symbol
A
Flammable and combustile material
8
Q
Open circles, open on the outside three circles WHMIS symbol
A
Biohazardous infectious material
9
Q
Pouring test tube on hand WHMIS symbol
A
Corrosive material
10
Q
“T” WHMIS symbol with a dot underneath
A
Poisonous and infectious causing other toxic effects
11
Q
What does WHMIS stand for?
A
Workplace, hazardous, material, information, systems
12
Q
Safety Hazard Symbols Naming
A
Flammable, toxic, explosive, irritant, corrosive, biological, electrical
13
Q
Safety hazard symbol: Flames
A
Flammable
14
Q
Safety hazard symbol: Skull
A
Toxic
15
Q
Safety hazard symbol: Rock crazy explosion thing
A
Explosive
16
Q
Safety hazard symbol: “X”
A
Irritant
17
Q
Safety hazard symbol: Hand in a chemical thing
A
Corrosive
18
Q
Safety hazard symbol: Three closed circles around another circle
A
Biological
19
Q
Safety hazard symbol: Lightning Strike
A
Electrical
20
Q
Name a few lab safety rules
A
Figure it out, look at the textbook idrc anymore
21
Q
Science class rules for before starting an activity
A
- Follow any safety instructions outlined by a teacher and in the textbook
- Identify possible hazards and report them immediately
- Show respect and concern for your safety as well as classmates and teachers
- Safety in the lab rules/section
22
Q
Matter
A
Anything that has mass and occupies space
23
Q
MSDS
A
Material, safety, data, sheets
24
Q
States of matter
A
liquid, gas, solid, (plasma)
25
What do states of matter depend on?
Temperature
26
Melting
Solid to liquid
27
Freezing
Liquid to solid
28
Evaporation
Liquid to gas
29
Condensation
Gas to liquid
30
Sublimation
Gas directly to solid
31
Deposition
Solid directly to gas
32
Properties
Characteristics that can be used to describe a substance
33
Matter has two types of properties...
Physical and Chemical
34
Physical properties
Can be used to identify matter
35
Physical Change
Appearance or state may be altered, but it's composition stays the same
36
Examples of physical properties
Colour, lustre, melting point, boiling point, hardness, malleability, ductility, crystal shape, solubility, density, conductivity
37
Example of a physical change
Melting, freezing idk guess
38
Define some physical properties (Understand what they are/do/mean)
Melting point: Temp that a substance changes from solid to liquid
Boiling point: temp that a substance changes from liquid to gas
Hardness: ability to resist being scratched
Malleability: Pounded or rolled into sheets
Ductility: Stretched into long wire
Crystal shape: Shape of a substances crystals
Solubility: ability to be dissolved in another substance
Density: amount of mass in a given volume
Conductivity: ability to conduct electricity or heat
39
Chemical Properties
Describes how a substance interacts with other substances. Observable only when a chemical change occurs
40
Chemical change
always results in the formation of different substance or substances. New properties.
41
Chemical properties examples
Reaction with acids, ability to burn, reaction with water, behavior with air, reaction with heat
42
All matter is either a...
Mixture or a Pure ("Pure") Substance
43
Pure Substance
Made up of only one kind of matter and has unique properties that set it apart from other types of matter. Can either be an element or a compound
44
Element
Material that cannot be broken any further, building blocks for all compounds
45
Compound
two or more elements combine chemically
46
Mixture
Combination of pure substances, do not combine chemiclaly. Remain in original, pure form.Four main types of mixtures.
47
Mechanical Mixture
Different substances that make up the mixture are visible
48
Solution
Different substances are not visible in a substances seperately
49
Solution examples/types
Solid in liquid, liquid in liquid, gas in liquid, gas in gas, solid in solid
50
Substances dissolved in water
Aqueous solution
51
Suspensions
Cloudy mixture in which tiny particles are held within one another. Can be seperated
52
Colloids
Cloudy mixture in which particles are so small they cannot be seperated easily
53
Physical Change
A material changes from one state to another. Can be changed back by adding or taking away energy.
54
Chemical Change
Two or more materials react and create new materials with new properties
55
Evidence of chemical changes
Odor, colour, formation of gas or solid release or absorption of heat energy
56
How is the periodic table organized
Increasing atomic mass
57
Atomic Mass
Mass of all protons and neutrons in the nucleus of an atom, electrons are so small they have no mass basically, measured in amu (atomic mass unit)
58
Dmitri Mendeleev
Organized the elements based on their properties, found a pattern that allowed him to predict elements that hadn't been discovered yet
59
Model of the atom
Electrons in the electron shells (2,8), protons and neutrons in the nucleus. Protons = electrons
60
Horitonzal rows in the periodic table
Periods 1-7
61
Vertical rows in the periodic table
Group/family 1-18
62
Mass number
The sum of the number of protons and neutrons in the atom
63
Metals
Shiny, malleable and ductile elements that conduct electricity. Found on the left side of the staircase
64
Non-Metals
dull, brittle, element that doesn't conduct electricity. Can be solid or gas at room temperature
65
Metaloids
Both metal and non-metal properties
66
Alkali Metals
Group 1 elements in the periodic
table. (NOT including Hydrogen). Most reactive of all the metals.. React when exposed to air or water!! As you move down the group the reactivity increases. What is the Most reactive??
67
Alkali-Earth Metal
Group 2 elements in the
periodic table. Reactivity is not as strong as the alkali metals.
68
Halogens
Group 17 elements in the periodic
table. Most Reactive Non-metals!!
69
Noble Gas
Group 18 elements in the periodic
table. The Most Stable and Unreactive elements on the
periodic table.
70
Chemical Formula
Combination of symbols that
represent a compound. It identifies the elements in the compound and the number of
atoms of each element in the compound.
71
Guyton de Morveau
Created a naming system for
compounds. To begin, if there is a metal in the compound it will always be first in the formula AND in the name. If you know the formula you can figure out the name and vice
versa.
72
No number next to the chemical formula
In the chemical formula, if there is no number next to the element symbol it means there is 1 atom of
that element!!
73
Physical state of the compound
Found in the brackets next to the formula
74
Ionic Compounds
Ionic compounds are always made by combining a metal (Na) and a non-metal (Cl). NaCl (s)
75
Properties of Ionic compounds
High boiling and melting points
Conduct electricity
Specific crystal shape e.g. salt crystals (NaCl)
Are solids at room temperature.
76
Ionic Bonds
Atoms of the elements are held together
77
Ion
An atom has a charge due to the gain or loss of electrons
78
Have unique names
Polyatomic ions
79
Naming ionic compounds
2 rules
1. the chemical name of the metal goes first ALWAYS!!....followed by the name of the non-metal.
2. the end of the name of the non-metal changes to “ide”
E.g. Chlorine becomes Chloride
Sodium and Chlorine becomes- “Sodium Chloride”
80
Exceptions to naming ionic compounds
1. If we are using polyatomic ions the name stays the same.
E.g. Carbonate stays as carbonate.
Calcium + Carbonate = “Calcium Carbonate”
2. If the metal has more than one choice of ion charge we must identify it in the name.
E.g. Fe+2 and O-2 becomes Iron (II) Oxide
E.g, Fe +3 and O -2 becomes Iron (III) Oxide
81
Using ion charges and chemical names to write formulas
Step 1 – Identify the charges on the elements
Mg+2, Cl-1
Step 2 – “balance” the ion charges so there are the same amount of +’s as –’s
Ca+2 ---- Cl-1 ---- Cl-1
1 atom of Ca and 2 atoms of Cl becomes.... CaCl2 (s)
82
Molecular compounds
Molecular compounds are formed when 2 or more NON-METALS are combined.
83
Molecular compounds properties
Can be liquid, solid or gas at room temp. Are insulators, poor electrical conductors and have
LOW boiling and melting points.
E.g. Water – H2O, Sugar – C6H12O6 (glucose)
84
Writing formulas
Similar to writing ionic formulas....but there are NO
ion charges to balance!!
Just need to interpret the compounds name to figure
out the number of each type of atom and the order of
elements!!
85
Naming molecular compounds
Many molecular compounds are known by their common name.
i.e. water (H2O), ammonia (NH3)
86
Rules for naming molecular compounds
ALL molecular compounds (except those containing
HYDROGEN) can be named using the following rules:
1. the first element in the compound uses the element
name – just like with ionic.
2. the second element in the compound has the suffix
“ide” – just like with ionic.
3. a PREFIX must be used to determine the number of
atoms of each element in the compound.
87
Naming rules for number of atoms/prefizes
1 – mono, 2 – di, 3 – tri, 4 – tetra, 5 – penta, 6 – hexa, 7
– hepta, 8 – octa, 9 – nona, 10 – deca.
88
Exceptions to naming compounds
**EXCEPTION – when the first element has one atom you DO NOT use the mono prefix**
PREFIX + first element PREFIX + second element +”ide”
89
Chemical reactions
A chemical reaction occurs when 2 or more substances combine to form new substances.
90
Materials at the beginning of a chemical reaction
Reactants
91
Materials at the end of a chemical reaction
Products
92
Evidence of a chemical change
Color change
Odor forms
Solid or gas is produced
Release or absorption of heat
93
Exothermic reactions
chemical reaction that
releases heat energy
Ex. when you burn anything
94
Endothermic reactions
chemical reaction that
absorbs heat.
Ex. Chemical Cold packs
95
Combustion reactions
Fast Chemical reaction that occurs when oxygen reacts with a substance to form a new substance and gives off energy.
Ex. Fire, car engine (internal combustion engine)
96
Corrosion
Slow chemical reaction that occurs when oxygen in the air reacts with a metal.
Ex. Rusting of the metal on a car
97
Cellular Respiration
Chemical reaction that takes place in the cells in your body to get energy from glucose.
Ex. Food (glucose) reacts with oxygen to produce energy, water, and carbon dioxide.
98
Conservation of mass
Matter is NOT created or destroyed in a chemical reaction, The TOTAL mass of reactants must equal the TOTAL mass of products!!
Ex. Fe (13.9g) + S (8.0g) → FeS (21.9g)
99
Closed system
Chemical reaction where material is not allowed in or out – All reactants and products are
accounted for.
Ex. Mg (24.3g) + S (32.1g) → MgS (?)
100
Open system
Chemical reaction where one or more products
can escape.
Ex. Alka seltzer (10g) + water (100g)→ water solution
(106g) + carbon dioxide (4g)
The CO2 has escaped as gas.
Ex. Gasoline + O2 + spark → energy + exhaust
All products escape!! – but if we could collect the exhaust its
mass would equal the gas used. (more or less...the energy
created cant be collected)
101
Factors affecting the speed of a chemical reaction
1. Catalysts
2. Concentration
3. Temperature
4. Surface Area
102
Catalysts
Any substance added that helps a
reaction go faster (usually not consumed during
the reaction)
Can be found in the living and non-living things.
Living – enzymes help us break down food faster.
Non-living – page 167 demo. (Manganese (IV) Oxide
catalyst)
103
Concentration
The greater the concentration of reactants, the faster the reaction – more atoms of reactants = more
reactions.
104
Temperature
If we add heat the atoms move faster = more collisions between more atoms of reactants = faster
reaction!
105
Surface Area
The more available surface area of reactants = the more area for collisions to occur = faster reaction!
Ex. What starts on fire faster? A large un cut log OR a large
log cut up into small pieces which increase surface area.
Ex. What dissolves faster? A sugar cube OR the same
amount of sugar uncubed in powder form? (this is not a
chemical reaction but you get the idea.)
