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Science 9 Unit 2 Atoms & Elements Exam > whole unit > Flashcards

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1
Q

Adhesion

A

The property of sticking to other substances; a physical property of water.

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2
Q

Chemical Change

A

The change in matter that results in the formation of a new substance or substances.

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3
Q

Chemical Property

A

A characteristic of a substance that describes its ability to change into a new substance or substances.

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4
Q

Chemical Reaction:

A

The process in which a chemical change occurs; a reaction that produces a new substance or substances.

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5
Q

Cohesion

A

The property of sticking together; a physical property of water.

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6
Q

Combustibility

A

The ability of a substance to react quickly with oxygen to produce heat and light energy.

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7
Q

Compound

A

A pure substance made from two or more elements that are combined together chemically.

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8
Q

Element

A

A pure substance that can’t be broken down into simpler substance.

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9
Q

Mass

A

The measurement of the quantity of matter in an object.

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10
Q

Matter

A

Anything that has mass and volume

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11
Q

Mechanical Mixture

A

A combination of pure substances in which the different substances are individually visible; a type of heterogeneous mixture

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12
Q

Medicine Wheel

A

A First Nations and Metis way of knowing the physical world; has four different quadrants and connects everything in the universe together into one whole.

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13
Q

Physical Property

A

A characteristic of a substance that can be observed or measured.

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14
Q

Property

A

A characteristic that describes a substance

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15
Q

Pure Substance

A

A substance made up of only one kind of particle, with a unique set of properties such as colour, hardness, boiling point, and melting point.

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16
Q

Solution

A

A combination of pure substances in which the different substances aren’t individually visible; a homogeneous mixture

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17
Q

Suspension

A

A cloudy mixture in which tiny particles of one substance are held within another; a type of heterogeneous mixture

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18
Q

Volume

A

A measurement of how big an object is or how much space a fluid takes up.

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19
Q

Anything that has mass and volume is…..

A

Matter

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20
Q

The state of matter where the atoms have the second lowest amount of energy is…..

A

Liquid

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21
Q

Elements and Compounds are examples of….

A

Pure Substances

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22
Q

The state of matter with the most energy is…

A

Plasma

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23
Q

When things stick to other substances it’s called…

A

Adhesion

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24
Q

When things stick to themselves it’s called…

A

Cohesion

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25
Q

A compound is an example of….

A

Pure Substances

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26
Q

A compound is an example of a….

A

Pure Substance

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27
Q

Trail mix would be an example of a….

A

Mechanical Mixture

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28
Q

The difference between a mixture and a compound is…

A

compounds are chemically combined but mixtures aren’t

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29
Q

What type of reaction is described: sulphur is yellow

A. Physical or B. Chemical

A

A. Physical

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30
Q

What is a chemical change?

A

It’s a change in matter that results in the formation of a new substance or substances.

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31
Q

Use an example to describe the difference between cohesion and adhesion

A

Due to cohesion, water forms beads on non-absorbent surfaces such as glass. With adhesion a towel is able to mop up water by using this property of water.

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32
Q

What are two physical changes that cooling a hot substance may result in?

A
  • Condensation

- Freezing

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33
Q

What’s the difference between an element and a compound?

A

An element is a pure substance made up of one type of particle that cannot be broken down into any simpler substance by chemical means. A compound is a pure substance that is made from two or more elements that are chemically combined.

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34
Q

Alkali Metals

A

elements found in Group 1 of the periodic table of elements; these metals have low melting points and react easily with water and air.

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35
Q

If water freezes inside of a building’s water pipes, the pipes may burst. Explain why this happens, in terms of a physical or chemical change.

A

It would be from a physical change. The pipe will burst because the water expands when frozen which will build up pressure on the pipe and it will then burst.

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36
Q

Substances can have a combination of materials in one or more states
~True or False

A

True

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37
Q

Alloy

A

A solution of two or more metals.

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38
Q

Atom

A

The smallest unit of an element that has all of the element’s properties.

39
Q

Atomic Mass

A

The average mass of an element’s atoms.

40
Q

Atomic Mass Unit

A

(amu) A unit of measure used to measure an atom’s mass.

41
Q

Atomic Number

A

The number of protons in an atom of an element.

42
Q

Atomic Theory

A

The theory that explains the nature of matter; study of the nature of atoms and how they combine to form all types of matter.

43
Q

Bond

A

The attraction between atoms or ions.

44
Q

Chemical Formula

A

A formula that identifies which elements, and how many atoms or ions of each, are in a compound.

45
Q

What is a chemical change?

A

A change in matter that results in the formation of a new substance or substances.

46
Q

Covalent Bond

A

The attraction between atoms created by the sharing of a pair of electrons between atoms.

47
Q

Diatomic Molecule

A

A molecule that contains two atoms of the same element.

48
Q

Electron

A

A negatively charged particle in an atom, located outside the nucleus of the atom.

49
Q

Group (Chemical Family)

A

One of 18 vertical columns in the periodic table of elements; classification of elements with certain shared physical and chemical properties.

50
Q

Halogens

A

Elements found in Group 17 of the periodic table of elements; these non-metals are all very reactive.

51
Q

Ion

A

An atom or group of atoms that has an electric charge as the result of losing or gaining electrons.

52
Q

Ion Charge

A

An electric charge that an atom or group of joined atoms take on when it loses or gains electrons.

53
Q

Ionic Bond

A

The attraction between ions of opposite charges; e.g, bond in an ionic compound.

54
Q

Ionic Compound

A

A pure substance formed when at least one metal and one non-metal combine chemically.

55
Q

Lattice

A

A regular, patterned three-dimensional structure.

56
Q

Law

A

A generalized description of some aspect of the physical world under certain conditions

57
Q

Mass number

A

The total number of protons and neutrons in the nucleus of an atom.

58
Q

Metalloids

A

Elements with metallic and non-metallic properties. Ex. Silicon

59
Q

Metals

A

Elements that are malleable and ductile, and conduct electricity and heat; most elements are metals

60
Q

Molecular Compound

A

A pure substance formed when non-metals combine chemically.

61
Q

Molecule

A

A group of atoms that share electrons; molecular compounds contain molecules.

62
Q

Neutral

A

The property of having no overall electric charge; both the positive and negative charges are equal.

63
Q

Neutron

A

A neutral particle in an atom, located in the nucleus of the atom.

64
Q

Noble gases

A

Elements found in group 18 of the periodic table of elements; these gases aren’t chemically reactive except in certain special situations.

65
Q

Non-metals

A

Elements that don’t resemble metals; non-metals are brittle and generally don’t conduct electricity or heat; ex carbon

66
Q

Nucleus

A

The centre of an atom where all the atom’s positive charge and most of an atom’s mass is concentrated.

67
Q

Period

A

One of the seven horizontal rows in the periodic table of elements.

68
Q

Periodic Table

A

A chart that organizes all of the elements in rows and columns.

69
Q

Proton

A

A positively charged particle in an atom, located in the nucleus of the atom

70
Q

Relative mass

A

The mass of an object in comparison to the mass of another object.

71
Q

Subatomic particle

A

A particle that makes up an atom; includes protons, neutrons, and electrons.

72
Q

Theory

A

A generalized explanation of a set of related observations or events supported by research and good arguments.

73
Q

Who proposed that everything is made up of tiny spheres?

A

Dalton

74
Q

He stated that electrons are in specific energy levels around the nucleus

A

Bohr

75
Q

He stated that an atom is a positively charged sphere with electrons scattered throughout.

A

Thompson

76
Q

He used charged particles in a experiment to determine protons are in a central mass.

A

Rutherford

77
Q

James Chadwick proposed the addition of neutrons in the nucleus. Who did he work with?

A

Rutherford

78
Q

Which of the three types of elements makes up majority of the periodic table?

A

Metals

79
Q

Which elements on the periodic table are known as semi-conductors?

A

Metalloids

80
Q

The vertical columns on the periodic table are known as…

A

Groups

81
Q

The horizontal rows on the periodic table are known as…

A

Periods

82
Q

A solution of two or more metals is called a(n)…

A

Alloy

83
Q

Is the most common element on Earths surface.

A

Oxygen

84
Q

Of the three categories that the periodic table can be split up into, these are the least common

A

Metalloids

85
Q

What do you call an atom that has lost or gained an electron?

A

Ion

86
Q

What group on the periodic table has a full valence shell?

A

Group 18

87
Q

What do scientists call the smallest possible amount of a pure substance that can exist?

A

An atom because they are in all elements and can’t be broken down any smaller.

88
Q

Define the word “compound”. Give an example.

A

A pure substance that’s made of two or more elements combined chemically. Ex. Water because it’s a combination of hydrogen and oxygen.

89
Q

Distinguish between “analytical” and “holistic” ways of thinking. Give an example of each.

A

Analytical thinking is the scientific way of thinking. Holistic thinking is a cultural belief about something. Ex. How they both differently view cancer.

90
Q

Based on the structure of ionic compounds, explain why they are usually hard solids with high melting points.

A

They consist of a metal and non-metal which both have high melting points and they’re usually solid.

91
Q

Describe each of the different models of the atom that have been created over time.

A

John Dalton- he said atoms were spheres.
J.J Thompson- he said they were spheres with positive and negative charges.
Ernest Rutherford- he added the nucleus to the model.
Niels Bohr- he added energy levels to the model.

92
Q

What type of elements are most often used in electronics? Why?

A

Metalloids because they’re semi-conductors

93
Q

Draw a Bohr diagram of 3 different elements.

A

Look it up or look in periodic table to check.

94
Q

Name some of the elements in the alkali metals, halogens, and noble gases groups.

A

Alkali metals- lithium, sodium
Halogens- chlorine, bromine, iodine.
Noble gases- silicon, oxygen, helium, neon.

Science 9 Unit 2 Atoms & Elements Exam (1 decks)

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