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Science 10: Chemistry > Chemistry: Quiz 1 > Flashcards

Chemistry: Quiz 1 Flashcards

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1
Q

Particle Model of Matter

A

All matter is made up of small particles called atoms
The particles in a substance are attracted to each other
All particles in a pure substance are the same
There are spaces between particles
Particles are always moving

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2
Q

Mass

A

Matter is anything that has mass and occupies space

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3
Q

Solids

A

Particles are tightly packed
Fixed (definite) volume and shape
Particles move very little

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4
Q

Liquids

A

Particles are farther apart than in a solid
Fixed (definite) volume and changing shape
Particles move around

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5
Q

Gases

A

Particles are loosely packed
Changing volume and shape
Particles move freely (need a lid for containers)

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6
Q

What are the different ways matter can change state

A

Solid → liquid: melting
Liquid → solid: freezing

Liquid → gas: vapourizing / evaporating
Gas → liquid: condensing

Solid → gas: subliming
Gas → solid: subliming

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7
Q

Physical Properties

A
  • Can be observed with the five senses
    Ex: shape, size, texture, flexibility, boiling point, melting point, state, how hard it is, magnetic, density
  • When a physical change occurs, the molecules do NOT change
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8
Q

Chemical Properties

A
  • Describes the reactivity of a substance
  • How a substance will react to other substances
  • A chemical change occurs when you create a new substance
    Ex: changes in smell or colour, how easily it catches fire or burns, how it reacts with other substances.
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9
Q

Pure Substance

A
  • All parts that make up the substance are identical
  • Its chemical and physical properties are constant
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10
Q

Elements (from the chart)

A
  • It is a substance made up of only one type of atom
  • Cannot be broken down into other substances
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11
Q

Compounds

A
  • A chemical combination of two or more elements in a specific ratio
  • Elements are held together by chemical bonds
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12
Q

Homogenous

A

A mixture in which the different substances are NOT visible

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12
Q

Colloid

A

A mixture in which the suspended substance cannot be separated from the other substances in the mixture

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13
Q

Mixture

A
  • A combination of pure substances
  • The proportions in a mixture vary, so the properties of the mixture vary
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14
Q

Heterogeneous

A

A mixture in which the different substances are visible

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15
Q

Suspensions

A

A mixture in which the components are in different states

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16
Q

Mechanical Mixture

A

A mixture in which the different substances are visible

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17
Q

John Dalton

A
  • All matter is made up of small, invisible particles called atoms
  • Described atoms as tiny spheres
  • All atoms of an element have identical properties such as size and mass
  • Atoms of different elements have different properties
  • Atoms of different elements can combine to form now substances (compounds)
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18
Q

J.J. Thomson

A
  • Discovered the electron (negative)
  • Atom was represented using the “plum pudding” or “raisin bun” model
  • His experiments showed that atoms of different elements contained smaller particles that were identical
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19
Q

Ernest Rutherford

A
  • Discovered the nucleus of the atom
  • Believed that most of the atom was empty space
  • The nucleus of the atom contained protons (positive) and neutrons (neutral)
  • The electrons orbited around the nucleus
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20
Q

Niels Bohr

A

Electrons travel only in specific electron shells or energy levels

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21
Q

Current Atomic Theories

A
  • Each level can be thought of as a cloud of negatively charged electrons
  • The electron cloud surrounds a nucleus containing two types of particles (neutrons and protons)
  • Electrons are grouped in pairs
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22
Q

Elements

A
  • Substances that cannot be broken down into other substances
  • The basic building blocks of all materials
  • 90 elements are naturally occuring, others are synthetic (created by humans using nuclear reactors, particle accelerators, or the atomic bomb
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23
Q

Atomic Number

A
  • Number that indicates the amount of protons in a particular element
  • The atomic number defines what the element is
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24
Q

Group (Families)

A
  • The vertical columns on the periodic table
  • There are 18 groups
  • Groups have similar chemical and physical properties
25
Q

Periods

A
  • The horizontal rows on the periodic table
  • There are 7 periods
  • Each period has the same number of energy levels
26
Q

Properties

A
  • Elements have certain properties / characteristics depending on whether they are a metal, non-metal or metalloid
  • Metals are on the left of the staircase
  • Non-metals are on the right
  • Metal are along the staircase
27
Q

Properties of Metals

A
  • Solid at room temperature (1 exemption: mercury)
  • Good conductors of heat and electricity
  • Shiny in appearance; can be polished
  • Malleable: can be hammered or rolled into thin sheets
  • Ductile: they can be stretched into a wire
28
Q

Properties of Non-Metal

A
  • Can be solid, liquid, or gas at room temperature
  • Poor conductors of heat and electricity
  • Dull in appearance
  • Brittle: breaks when hammered
  • Not ductile
29
Q

Metalloids

A

Share some properties of both metals and nonmetals

30
Q

Alkali Metals

A
  • Metals in the first column or group 1
  • With the exception of francium, these metals are very soft and shiny and silvery
  • These elements react vigorously, event violently, with water and must be stored in oil to prevent contact with the moisture in the air
31
Q

Alkaline - Earth Metals

A

Metals in the second column of group 2
These elements are shiny, silver but not as soft as the alkali metals
Their compounds tend to be white

32
Q

Halogens

A
  • The reactive nonmetals in group 17 of the periodic table
  • These elements are so reactive that they are never found as elements in nature
33
Q

Noble Gases

A
  • Elements belonging to group 18
  • These elements are very unreactive
34
Q

Subatomic Particles

A
  • Protons
  • Neutrons
  • Electrons
35
Q

Atomic Mass

A
  • The mass of an average atom of the element
  • The total number of protons and neutrons
  • Protons and neutrons gather together in the nucleus of the atom
  • This number may be slightly different depending on which periodic table you are looking at.
36
Q

Calculating th emost common number of neutrons in an atom

A
  • Atomic mass on the periodic table is the most common (average) mass of one atom of that element (they can vary)
  • The number of protons never changes and is the same as the atomic number

Number of neutrons = atomic mass - atomic number

37
Q

Isotopes

A

Since the number of neutrons can vary, atoms of the same substance with different numbers of neutrons are called isotopes

38
Q

Charge

A
  • Atoms have no net charge
  • The number of protons = the number of electrons
  • The atomic number tells you how many electrons and protons are in an atom
39
Q

Electron Clould

A
  • Space in which electrons orbit the nucleus at high speed
  • Within the clouds are energy levels
40
Q

Energy Levels

A
  • Areas where electrons orbit the nucleus
  • Each level can fit a certain number of electrons (octet rule)
41
Q

Valence Electron

A

Electrons in the outer energy level are known as valence electrons. Elements in the same group have the same number of valence electrons.

42
Q

Ions

A
  • Atoms want to have a stable (full) outer energy level
  • To become stable the atoms will gain or lose (whichever is easiest) valence electrons to ensure their outer level is full
  • These electrons are transferred to other ions (forming compounds)
  • Gain or loss of electrons causes the atom to have a charge
43
Q

Positive Ions

A
  • When an ion loses electrons it becomes positively charged
    - All metals are
    positively charged
    - Positively charged ions
    are called cations (cats
    have paws)
44
Q

Negative Ions

A
  • When an ion gains electrons it becomes negatively charged
    - All non-metals are
    negatively charged
    - Negatively charged
    ions are called anions
45
Q

The International Union of Pure and Applied Chemistry (IUPAC)

A

The group responsible for naming compound

46
Q

Molecular Compounds

A
  • Are formed when 2 or more nonmetals share electrons in their outer energy level to become stable
  • The bonds formed when electrons are shared are called covalent bonds
  • The bond formed is not as strong as an ionic bond
47
Q

Molecular Elements

A
  • Form molecules made up of only one type of atom
  • Have the same name as the element
  • The special seven
48
Q

The Special Seven

A
  • These seven elements form diatomic molecules when they are individually writing (H2, N2, O2, F2, Cl2, Br2, I2)
  • Two other polyatomic molecules are sulphur (S8) and phosphorous (P4)
49
Q

Ionic Compounds

A
  • Formed when electrons are transferred from a metal to a non-metal
  • Creates an ionic bond between a cation (positive ion) and an anion (negative ion)
  • Cations donate electrons to anions as they form a molecule
  • The ratio of positive charges to negative charges must be zero
50
Q

Polyatomic Ions

A
  • Ions made up of a group of atoms acting as ONE UNIT
  • Held together with covalent bonds
51
Q

Multivalent Elevents

A
  • Multivalent elements form ions that can have more than charge
  • They are listed on the periodic table for you
  • The first charge listed in the most common
52
Q

Water

A

H2O

53
Q

Hydrogen Peroxide

A

H2O2

54
Q

Ammonia

A

NH3

55
Q

Sucrose

A

C6H12O11

56
Q

Glucose

A

C6H12O6

57
Q

Methane

A

CH4

58
Q

Propane

A

C3H8

59
Q

Methanol

A

CH3OH

60
Q

Ethanol

A

C2H5OH

61
Q

Hydrogen Sulfide

A

H2S

Science 10: Chemistry (1 decks)

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