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Science grade 9 exam cards > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

Chemical properties

A

Any properties that describe how a substance reacts with another substance

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2
Q

Compound

A

different elements combined in definite proportions

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3
Q

density

A

mass of a substance to the volume it occupies

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4
Q

Electron

A

can only move within fixed energy levels (negatively charged)

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5
Q

Element

A

made up of only one kind of particle called atom.

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6
Q

Group (families)

A

columns (up and down) that represent the number of electrons in the outermost energy levels

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7
Q

Homogenous

A

Evenly combined or mixed substances

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8
Q

Heterogenous

A

Unevenly combined or mixed

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9
Q

Ions

A

atoms can gain or lose electrons producing charged particles

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10
Q

Isotope

A

members of a family of an element that all have the same number of protons but different numbers of neutrons

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11
Q

Ionic compound

A

a metal and non-metal element bonded together

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12
Q

Lustre

A

shiny, dull surface

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13
Q

Metalloid

A

an element that share some properties of both, metals and nonmetals

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14
Q

Mixture

A

composed of two or more substances

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15
Q

Malleability

A

ability to be hammered into a sheet

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16
Q

Matter

A

anything that has a mass and occupies space

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17
Q

Metal

A

an elements that is typically hard shiny, and a conductor of electricity

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18
Q

Molecular compound

A

two nonmetals bonded together

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19
Q

Neutron

A

neutral (no charge) sub-atomic particle

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20
Q

Non-metal

A

typically, an element that is not shiny, most an not visible and are poor conductors

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21
Q

Period

A

rows (right to left) on the periodic table that represents the number of energy levels

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22
Q

Physical properties

A

something that can be observed or measured without changing the type of matter

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23
Q

Pure substance

A

matter that is made up of only one type of particle and cannot be separated physically (made of elements and compounds)

24
Q

Proton

A

positively charged sub-atomic particle

25
Q

Solubility

A

the ability of a substance to dissolve in another substance

26
Q

Solution

A

a homogenous type of mixture of two or more substances

27
Q

Texture

A

smooth, rough surface

28
Q

Give two examples of chemical properties that can be used to describe matter.

A

Flammability, reaction with other substances

29
Q

Give two examples of physical properties that can be used to describe matter.

A

Solid: holds it shape, fixed volume, molecules packed tightly
Liquid: takes the shape of its container, fixed volume, Molecules slide past each other
Gas: takes the shape of its container, volume of container, molecules are far apart

30
Q

Provide 2 examples of a Homogeneous Mixture

A

Juice, water + salt

31
Q

Provide 2 examples of a Heterogeneous Mixture

A

Pizza, sandwich

32
Q

Provide 2 examples of an Element

A

Sodium (Na), Hydrogen(H)

33
Q

Provide 2 examples of a compound

A

Carbon dioxide (CO2), Water(H2O)

34
Q

What type of charge does an electron have, and where is it located in an atom

A

It has a negative (-) charge and it is located outside the nucleus

35
Q

What type of charge does a proton have, and where is it located in an atom

A

It has a positive (+) charge and it is located inside the nucleus

36
Q

What type of charge does a neutron have, and where is it located in an atom

A

It has no charge (0) and it is located inside the nucleus

37
Q

How does an atom become an ion?

A

An atom can gain or lose electrons producing charged particles called ions

38
Q

If an atom gains two electrons, what charge does it have?

A

The atom will have a 2- charge

39
Q

How does an atom become an ion with a charge of +3

A

The atom is positively charged

40
Q

What is the equation of density?

A

D = M/V

41
Q

Provide the name for each of the following groups in the periodic table and identify one characteristic of each

A

Group 1: The alkali metals; want to lose one electron to become a full outer shell
Group 2: The alkaline earth metals; All have two valence electrons
Group 17: The Halogen metals; want to gain one extra electron to have a full outer shell
Group 18: Group 18: The noble gases; Do not want to gain or lose electrons

42
Q

Dalton’s atomic theory

A

All matter is made up of small particles called atoms
Atoms cannot be created or destroyed
All atoms of the same element are identical in size or mass
Atoms of one element are different in mass and size from the atoms of other elements
Compounds are created when atoms of different elements are linked to definite proportions

43
Q

Thomson’s atomic theory

A

Noticed similar behaviour for different types of gases
Concluded that negatively charged particles are found in all matter and called them electrons
Knew that the atom had an overall neutral charge
Positively charged sphere with mostly empty space has negatively charged electrons throughout
“Raisin bun model”

44
Q

Rutherford’s atomic theory

A

Discovery of the nucleus
An atom contains a small dense , positively charged nucleus, surrounded by negatively charged electrons
Gold-Foil experiment

45
Q

Bohr’s atomic theory

A

Discovery of energy levels
Suggested that electrons existed in distinct energy levels

46
Q

What is an isotope?

A

An isotope is one of two or more forms of an element that have the same number of protons but a different amount of neutrons

47
Q

What the difference between ionic and molecular compounds?

A

Molecular compounds share electrons. While ionic compounds transfer electrons.

48
Q

Show how calcium and fluorine form a compound. Is it ionic or molecular? Write the chemical formula and name the compound that form.

A

Calcium fluoride. It is a ionic compound. CaF2

49
Q

Show how carbon and fluorine form a compound. Is it ionic or molecular? Write the chemical formula and name the compound that form.

A

Carbon Difluoride. It is a molecular compound. CF2

50
Q

Series circuit equation for current

A

Is = I1 = I2 = I3

51
Q

Series circuit equation for potential difference

A

Vs +V1 +V2+ V3

52
Q

Series circuit equation for resistance

A

Req = R1+ R2 + R3…
(the equivalent resistance is greater than the resistance of each individual resistor)

53
Q

Parallel circuit equation for current

A

Is = I1 + I2 + I3

54
Q

Parallel circuit equation for potential difference

A

Vs = I1 = I2 = I3

55
Q

Parallel circuit equation for resistance

A

1/Req = 1/R1 + 1/R2 + 1/R3…
(The equivalent resistance is smaller than the resistance in the smallest resistor)

Science grade 9 exam cards (4 decks)

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