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Chemistry 10 > Chem unit test > Flashcards

Chem unit test Flashcards

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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
Q

Metalloids

A
  • have properties that resemble both metals and non-metals.

- Can conduct energy but not well

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26
Q

Horizontal rows (on periodic table)

A

periods (1-17)

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27
Q

Vertical rows (on periodic table)

A

families or groups (1-18)

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28
Q

Group #1 (on periodic table)

A

Alkali Metals

  • lithium, sodium, potassium, rubidium, cesium, francium
  • soft, skinny, silver, in colour
  • very reactive with water
  • 1+ charge cations
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29
Q

Group #2 (on periodic table)

A

Alkaline Earth Metals

  • skinny, typically white in colour
  • less soluble than alkali metals
30
Q

Group #3-12 (on periodic table)

A

Transition Metals

  • Generally hard and dense
  • less reactive than alkali metals
31
Q

Group #17 (on periodic table)

A

Halogens

  • poisonous
  • reacts with alkali metals to form salts ex. sodium+chlorine= table salt
32
Q

Group #18 (on periodic table)

A

Nobel gases

-Very un-reactive (inert gasses)

33
Q

Third Isotope

A

has 1P and 2N

34
Q

How to get the # of neutrons (isotopes)

A

-Mass number - atomic number (protons)

35
Q

Molecular compounds

A
  • 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
Q

Naming molecular compounds

A

prefix + first element (never use mono)
-Prefix and second element and change ending to ide
EX- Dinitrogen monoxide

37
Q

Prefixes

A 
1-mono
2-di
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octa
9-nona
10-deca
38
Q

IUPAC

A

International Union of Pure and Applied Chemistry

39
Q

Forming Compounds

A

-Elements are most stable when their outer most energy level is full

40
Q

Valence Electrons

A

The electrons in the outer most level

41
Q

Naming Ionic Compounds

A

Name Cation first w/capital
Name anion second with lower case
Add ending to “ide” to the anion

42
Q

Ionic Compound

A
  • composed of an equal number of positive and negative charges
  • charges of cations must be equal to the total charge of anions
43
Q

Multivalent Ions

A
  • Transition metals
  • some metals have more than one stable ion
  • Roman numerals after a metals name indicates which ion it is
44
Q

Naming Multivalent Ions

A

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
Q

Polyatomic Ions

A

-ionic compounds composed of one or more non-metals

46
Q

Naming polyatomic ions

A

1-Name cation first w/capital letter
2-name the polyatomic anion
3-no name change in the polyatomic anion

47
Q

Solubility

A

How well a solid dissolves in a liquid
High solubility–> dissolves well
low solubility–> does not dissolve well

48
Q

Acids

A
  • 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
Q

naming acids

A

Hydrogen –> hydro

adds non metal –> hydrochloric

50
Q

Bases

A
  • pH greater than 7
  • may contain 0H ion + metal or NH4
  • tastes bitter
  • feels slippery
  • corrosive
  • turns red litmus paper blue
  • conducts electricity
51
Q

Neutralization

A
  • Acid + Base (adding them together)

- Both properties disappear

52
Q

Buffer

A

-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
Q

Indicators

A

-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
Q

Stomach Acid

A

IS very strong

55
Q

When do chemical reactions occur

A

When bonds between atoms are formed or broken

56
Q

Reactants

A

these are the substances that react

57
Q

Products

A

These are the new substances made by the reactants (they balance each other out)

58
Q

Evidence for chemical reaction

A
  • Gas is produced
  • precipitate is formed
  • a permanent colour change is observed
  • an energy change occurs
59
Q

Exothermic Reactions

A 
Releases energy (reacts to produce energy) 
EX- Handwarmers
60
Q

Endothermic Reactions

A

Uses/absorbs energy (produces product)

EX- Cold packs

61
Q

Antane Lavoisier

A

The total mass of all the reactants equal the total mass of all the products
EX- 15+15+30

62
Q

Chemical Equations

A
  • shows the conversion of reactants into products and their relative amounts
  • The front numbers are called coefficients
63
Q

Balancing Equations

A
  • 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
Q

Simple Composition

A

Two elements combine and form a compound
A +B =AB
Reactant + Reactant = product

65
Q

Simple Decomposition

A

A compound breaks up into it’s elements or simpler compounds
AB=A+B
Reactant=product+product

66
Q

Single Replacement

A

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
Q

Double replacement

A

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
Q

Hydrocarbon Combustion

A

occurs when a hydrocarbon reacts with oxygen gas

69
Q

Molar mass

A

g/mol

70
Q

How to get molar mass

A

m/n (mass divided by number of moles)

71
Q

How to get number of moles

A

m/M (mass divided by molar mass)

72
Q

How to get mass

A

n x M ( number of moles times molar mass)

Chemistry 10 (1 decks)

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