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Science 9 EXAM REVIEW > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

Qualitative property

A

a substance that isn’t measured and does not have numerical value.

Colour, odour & texture

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2
Q

Quantitative property

A

a substance measured through numerical value, height and mass.

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3
Q

What is matter?

A

is anything that has mass and takes up space

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4
Q

What are some examples of matter?

A

anything that takes up space
ex. air, rocks, water

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5
Q

What are some examples of things that aren’t matter?

A

Light, Time, Sound & Gravity

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6
Q

What is the particle theory?

A
  • All matter is made up of tiny particles separated by empty space
  • Different substances are made of different particles
  • All particles are in constant motion
  • Particles in a substance move faster as temperature increases
  • Particles attract each other
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7
Q

What is a pure substance?

A

Substances that are made up of only one kind of particle and have a fixed or constant structure.

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8
Q

What is a solution?

A

a uniform mixture of two or
more substances

(looks like a pure substance but it contains more than one type
of particle. clear apple juice)

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9
Q

What is a heterogenous mixture?

A

two or more substances that are physically combined and could be seperated by physically means visible differences

cereal + milk
pizza + toppings

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10
Q

What is a homogenous mixture?

A

mix of 2 or more pure substances that mix well together where it dissolves within eachother

ex. sugar + water

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11
Q

What are examples of a pure substance?

A

Tin, Sulfur, Diamond, Water, Sucrose (sugar), sodium chloride (salt), and baking soda (sodium bicarbonate)

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12
Q

What are examples of a solution?

A

Salt water, Sugar water, Mouthwash, Soda, Air, Acetone, Coffee, Lemonade, and Tea.

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13
Q

What are examples of heterogenous mixtures?

A

Hot Chocolate, Sand in water, toothpaste, mixed nuts, trail mix, pizza, etc.

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14
Q

What are examples of homogenous mixtures?

A

Air, Sugar water, Rainwater, Vinegar, Coffee, Detergent, Cologne, etc.

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15
Q

What is ductility?

A

A physical property of a material that describes its ability to be stretched, pulled, or drawn into a thin wire or thread without breaking.

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16
Q

What is luster?

A

How a mineral’s surface reflects light and how the interior of the material may refract/reflect or bend light.

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17
Q

What is density?

A

The measurement of how tightly a material is packed together.

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18
Q

What is flammability?

A

A measurement of how quickly a specific material is capable of catching fire and burning.

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19
Q

What is malleability?

A

The quality of something that can be shaped into something else without breaking

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20
Q

What is combustibility?

A

A measurement of how easily a substance bursts into flame, through fire, or explosion.

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21
Q

What is reactivity?

A

The ability of a substance to interact chemically with a second substance.

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22
Q

What is odour?

A

The smell of a substance

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23
Q

What is texture?

A

The feel, appearance or consistency of a surface or substance.

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24
Q

What is sollubility?

A

The ability to be dissolved

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25
Q

What is boiling point?

A

When water (any liquid) reaches over 100 degrees celsius.

CREATES GAS * WATER VAPOUR

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26
Q

What are examples of qualitative properties?

A

Hardness, Malleability, Electrical Conductivity, Sight, Taste, Smell, Touch.

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27
Q

What are examples of quantitative properties?

A

Temperature, Height, Mass, Volume, Density

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28
Q

What is a mixture?

A

A substance made from composing two or more substances together.

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29
Q

What are the similarities of Pure substances & Mixtures?

A

They are both matter and composed of Atoms, They also have weight, volume, and color

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30
Q

What are the similarties between Homogenous and Heterogenous?

A

Both are mixtures

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31
Q

What are the similarities between Qualitative and Quantitative substances?

A

They both are observations which are made from one substance to gather information.

32
Q

What is the difference between physical and chemical change?

A

A physical change only changes the appearance of the matter and not the substance.

However, chemical change creates a new substance with different properties and is not reversible.

33
Q

What is aristole’s theory of matter?

A

Theorized, Matter was made from 4 elements, Water, Air, Fire, and Earth.

34
Q

What is Democritus’ theory of matter?

A

Theorized that matter is composed of tiny invisible particles called atoms.

“INDIVISIBLE PARTICLE (ATOM)”

showed that atoms are the smallest unit of measurement

  • atoms are of different sizes
  • atoms are in constant motion
  • seperated by empty spaces (the void)
35
Q

What is Dalton’s Atomic theory?

A

“Billiard Ball Model”

  • all matter made up of indivisible particles called ATOMS
  • all atoms of an element are identical, and atoms of a different element are different
  • atoms can be rearranged but never created or destroyed

( Dalton’s model couldn’t explain attraction between objects )

36
Q

What is JJ. Thompson theory?

A

“Plum pudding model” aka ^chocolate chip muffin model

  • discovered negative particles are called ELECTRONS
  • theorized the rest of the atom is a positvely charged sphere

-said Atoms were positively charged with electrons spread throughout suggesting they had subatomic components.

37
Q

What device did J.J Thompson use to conduct his experiment?

A

Cathode ray tube

the particles he detected were attracted to the positive end of the circut so it had to be negatively charged

38
Q

What theory did Niels Bohr propose?

A

“Planetary model of an atom”
(how things orbit eachother in an atom)

  • electrons orbit the nuclus
  • electrons in an orbit have potential energy, farther away from nucleus = more energy
  • electrons can jump between orbits

(2, 8,8)

39
Q

What theory did James Chadwick propose?

A
  • Discovered neutrons
40
Q

What is a isotope?

A

Variation of the same element with a different number of electrons in their nucleus.

An atom with the same number of protons but different number of neutrons

(must be same element)

41
Q

What is atomic mass?

A

represents the mass of an atom

( # of protons + # of neutrons )

42
Q

Why do different isotopes have different atomic masses?

A

Different isotopes have different atomic masses because the number of neutrons is different.

43
Q

What are Covalent Bonds?

A

“molecular bonds”

Form between two nonmetals.

One or more electrons are shared between atoms forming a bond.

Atoms can share multiple pairs of electrons in double and triple bonds.

44
Q

What theory did Ernest Rutherford propose?

A

“Gold foil experiment”

  • DISCOVERED THE NUCLEUS
  • predicted the presence of positively charged particle called PROTONS
45
Q

Example of halogens?

A

poisonous things, chlorine.

bromine added to lightbulbs to increase brightness and operating life

46
Q

Why does aerosol explode in fire?

A

Aerosol explodes in fire because of heat, the product expands and the pressure is added onto the walls of the cans which then explode because of the sudden temperature change.

47
Q

What is chemical change & example?

A

A chemical change is when a substance changes and reacts with another substance such as iron rusting, burning wood, or fireworks.

48
Q

What is physical change & example?

A

A physical change is when no new substance is formed and involves melting, shredding, dissolving, boiling, chopping, etc.

49
Q

What are signs that a physical change has taken place?

A

The physical change includes changes in size, shape, or state, and no new substances are formed.

50
Q

What are signs that a chemical change has taken place?

A

The signs of a chemical property are that the substance is not reversible, colour change, odor change, and a new substance is formed

51
Q

What are examples of akali metals?

A

Potassium in plants and foods (bananas, oranges, e.t.c)

52
Q

What are examples of akaline earth metals?

A

Magnesium in fireworks
(akaline earth metals burn with a bright flame)

53
Q

What are examples of noble gases?

A

low density of helium used in balloons so it could float

54
Q

What are the properties of an element and who was this determined by?

A

Dmitri Mendeleev (1834-1907)

  • Atomic Mass
  • Density
  • Colour
  • Melting point
  • Boling point
55
Q

What is Mendeleev’s periodic law?

A

“If the elements are arranged according to their atomic mass, a pattern could be seen in which similar properties occur regularly”

56
Q

Noble Gases

A

Group 18

Valence Electrons: full shell
(prevents gases from forming compounds)

Very stable due to their max electrons in the outershell

57
Q

Rare earth metals

A

located at the bottom of a periodic table

58
Q

Halogens

A

Group 17

Valence electrons: 7
bonds easily with alkali metals
all nonmetals

“SALT FORMER” - very reactive non-metals & forms salt when reacting w metals

59
Q

Transition metals

A

Group 3 - 12

Valence Electrons: may vary

Properties: Ductile, Malleable, conduct electricity and heat

60
Q

Alkaline Earth Metals

A

Group 2

Very reactive

Valence Electrons: 2
can easily bond with other elements by losing these electrons

Not found free in nature

61
Q

What are alkali metals?

A

Group 1

Very reactive metals that do not occur freely in nature

Valence Electrons: 1

Properties: Malleable, Ductile, good conductors of heat & electricity, softer than most

Can explode if exposed to water

62
Q

What are the 7 Diatomic Molecules?

A

Hydrogen, Nitrogen, Fluoride, Oxygen, Iodine, Chlorine, Bromine

( Have No Fear Of Ice Cold Beer )

Two same elements bonded together, 7 of these Diotomic elements always exist in pairs of 2. (power to 2)

63
Q

What is a chemical family?

A

column of elements with similar properties on the periodic table
(belong to same group)

64
Q

What are metalloids?

A

Located along the staircase line

Have properties of both metals and non-metals

  • important use in digital electronices

-typically increases in conductivity as temperature increases

65
Q

What is the only non-metal liquid?

A

Bromine (element 35)

66
Q

What are non-metals?

A

Found in the upper right portion of the periodic table

Mostly gases and dull powdery solids

Does not conduct heat or electricity

67
Q

What is a metal element?

A

Located on left & central parts of the periodic table

solids which display a metallic lustre

(lustrous, malleable, ductile, conducts heat & electricity)

68
Q

What is an example of a compound?

A

Water ; (not an elements but is made up of two elements in the periodic table)

made with: Hydrogen & oxygen

69
Q

What is a compound?

A

A pure substance composed of two or more DIFFERENT elements that are chemically joined

70
Q

What is an element symbol?

A

an abbreviation for a chemical element

71
Q

What is an example of an element?

A

Silver, as it cannot carry out any chemical or physical reactions where silver will convert into something simpler

72
Q

What is an element?

A

A pure substance that cannot be broken down into simpler chemical substance by any physical or chemical means

! the building blocks of all substances and arranged on the periodic table

(things on the periodic table)

73
Q

Examples of chemical properties

A

Reactivity with water, flammability, acidity, and toxicity.

74
Q

Examples of physical properties

A

Colour, Lusture, opacity, Length, Volume, hardness, density, brittleness, viscosity, malleability, ductility, conductivity.

75
Q

What are ionic bonds

A

Science 9 EXAM REVIEW (4 decks)

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