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Chemistry 10 > Chem unit test > Flashcards

Chem unit test Flashcards

(72 cards)

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1
Q

What is chemistry about

A

is all about making things better

         ex. aspirin makes pain go away
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2
Q

What does cooking create

A

chemical changes in the interactions of heat, sugar and proteins in foods

  - heating/freezing 
  - salting 
  - fermentation
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3
Q

Metallurgy

A

study of physical and chemical properties of metal

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4
Q

alchemy

A
  • combination of science and magic

- no scientific method used

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5
Q

Who developed hypotheses about matter

A

Aristotle and the Democritus

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6
Q

Aristotle

A
  • Believed that all matter was composed of combinations of elements (earth, fire, water, air)
  • very well known so everyone believed him
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7
Q

Democritus

A
  • all matter was made up of tiny particles that could not be divided into smaller pieces (indivisible atomos)
  • not many people believed him even though he was correct
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8
Q

3 subatomic particles

A

protons have a positive charge
neutrons have no charge
electrons have a negative charge

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9
Q

what are found in the nucleus of an atom

A

protons and neutrons

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10
Q

what is the mass number

A

The sum of protons and neutrons

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11
Q

Isotopes

A

isotopes of atoms have the same number of protons but different numbers of neutrons.
EX- most hydrogen atoms have 1 proton but zero neutrons.
-1/100000 hydrogen atoms have 1 proton
and 1 neutron
-Each isotope has a different mass number (#of P + #of N)

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12
Q

Atomic Theory

A
  • smallest part of an element that still has all the properties of that element
  • protons and neutrons are 99.9% of the mass of an atom
  • most of the atom is empty space
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13
Q

Atomic number

A

refers to the number of protons

-all atoms of the same element have the same amount of protons

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14
Q

Energy levels of energy

A
  • like the bohr diagram
  • electrons closest to the neutrons are held tightly and have little energy
  • outer electrons are easier to let go of (lots of energy so can easily escape)
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15
Q

ion

A

atom that has lost or gained an electron

  • becomes electrically charged
  • ionization happens because an unfilled shell is unstable
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16
Q

cations

A
  • positively charged ions
  • formed when an atom losses an electrons
  • metals
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17
Q

anions

A
  • negatively charged ions
  • formed when an atoms gains an electron
  • non metals
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18
Q

Ionic compounds

A

a non metal + a metal

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19
Q

smallest to largest :compound, atom, element

A

atom, element, compound

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20
Q

Example of Ions

A

Sodium (Na) and Chlorine (Cl)

  • sodium will give up an electrons and give it to chlorine
  • Will name NaCl (sodium chloride)
  • metal name first, then non-metal name, then ide at end
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21
Q

Metals

A
  • shinny
  • grey/silver
  • good conductors of electricity
  • malleable (ability to be shaped)
  • ductile (ability to be stretched)
  • most are solid at room temp (except mercury L)
  • some react strongly with others
  • some are inert do not react with anything except strong acids (ex.gold)
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22
Q

Inert

A

inactive

ex- argon-argos (lazy)

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23
Q

Alloy

A

mixture/combination of two or more metals

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24
Q

Non-metals

A
  • 17 of the elements
  • 11 gases, 5 solids, 1 liquid
  • not reactive
  • cannot conduct energy
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25
Metalloids
- have properties that resemble both metals and non-metals. | - Can conduct energy but not well
26
Horizontal rows (on periodic table)
periods (1-17)
27
Vertical rows (on periodic table)
families or groups (1-18)
28
Group #1 (on periodic table)
Alkali Metals - lithium, sodium, potassium, rubidium, cesium, francium - soft, skinny, silver, in colour - very reactive with water - 1+ charge cations
29
Group #2 (on periodic table)
Alkaline Earth Metals - skinny, typically white in colour - less soluble than alkali metals
30
Group #3-12 (on periodic table)
Transition Metals - Generally hard and dense - less reactive than alkali metals
31
Group #17 (on periodic table)
Halogens - poisonous - reacts with alkali metals to form salts ex. sodium+chlorine= table salt
32
Group #18 (on periodic table)
Nobel gases | -Very un-reactive (inert gasses)
33
Third Isotope
has 1P and 2N
34
How to get the # of neutrons (isotopes)
-Mass number - atomic number (protons)
35
Molecular compounds
- solid, liquid or gas - low melting point - no crystal shape - do not conduct electricity - can be made up of multiple elements or the same element - share electrons and do not transfer them (covalent bond) - Non metal + non metal
36
Naming molecular compounds
prefix + first element (never use mono) -Prefix and second element and change ending to ide EX- Dinitrogen monoxide
37
Prefixes
``` 1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hepta 8-octa 9-nona 10-deca ```
38
IUPAC
International Union of Pure and Applied Chemistry
39
Forming Compounds
-Elements are most stable when their outer most energy level is full
40
Valence Electrons
The electrons in the outer most level
41
Naming Ionic Compounds
Name Cation first w/capital Name anion second with lower case Add ending to "ide" to the anion
42
Ionic Compound
- composed of an equal number of positive and negative charges - charges of cations must be equal to the total charge of anions
43
Multivalent Ions
- Transition metals - some metals have more than one stable ion - Roman numerals after a metals name indicates which ion it is
44
Naming Multivalent Ions
1-Name cation first starting with Capital 2-Name anion second 3-change ending to "ide" 4-use lower case letter with anion 5-write roman numeral after cation to indicate charge
45
Polyatomic Ions
-ionic compounds composed of one or more non-metals
46
Naming polyatomic ions
1-Name cation first w/capital letter 2-name the polyatomic anion 3-no name change in the polyatomic anion
47
Solubility
How well a solid dissolves in a liquid High solubility--> dissolves well low solubility--> does not dissolve well
48
Acids
- Solution that has a pH less than 7 - Contains H+ ions - tastes sour - corrosive - reacts with metal - turns blue litmus paper red - conducts electricity
49
naming acids
Hydrogen --> hydro | adds non metal --> hydrochloric
50
Bases
- pH greater than 7 - may contain 0H ion + metal or NH4 - tastes bitter - feels slippery - corrosive - turns red litmus paper blue - conducts electricity
51
Neutralization
- Acid + Base (adding them together) | - Both properties disappear
52
Buffer
-substance that keep s the pH of a solution nearly constant despite the addition of a small amount of acid or base EX- liming (alkaline) (adds calcium carbonate to a lake that has been affected by acid rain)
53
Indicators
-change colour depending on the pH of a solution EX- Litmus paper -universal indicator (large range of colour in response to different pH range) -Indicator labs
54
Stomach Acid
IS very strong
55
When do chemical reactions occur
When bonds between atoms are formed or broken
56
Reactants
these are the substances that react
57
Products
These are the new substances made by the reactants (they balance each other out)
58
Evidence for chemical reaction
- Gas is produced - precipitate is formed - a permanent colour change is observed - an energy change occurs
59
Exothermic Reactions
``` Releases energy (reacts to produce energy) EX- Handwarmers ```
60
Endothermic Reactions
Uses/absorbs energy (produces product) | EX- Cold packs
61
Antane Lavoisier
The total mass of all the reactants equal the total mass of all the products EX- 15+15+30
62
Chemical Equations
- shows the conversion of reactants into products and their relative amounts - The front numbers are called coefficients
63
Balancing Equations
- Adds the coefficients to show conservation of mass - equal number of molecules on each side - total mass of all the reactants = the total mass of all the products (they balance each other)
64
Simple Composition
Two elements combine and form a compound A +B =AB Reactant + Reactant = product
65
Simple Decomposition
A compound breaks up into it's elements or simpler compounds AB=A+B Reactant=product+product
66
Single Replacement
One element replaces another in a compound. A metal can replace a metal OR a nonmetals can replace a non-metal A +BC=AC + B
67
Double replacement
A metal replaces a metal or a nonmetal replaces a nonmetal in a compound (more than one element gets replaced) AB+CD=AD+CB
68
Hydrocarbon Combustion
occurs when a hydrocarbon reacts with oxygen gas
69
Molar mass
g/mol
70
How to get molar mass
m/n (mass divided by number of moles)
71
How to get number of moles
m/M (mass divided by molar mass)
72
How to get mass
n x M ( number of moles times molar mass)

Chemistry 10 (1 decks)

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