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Science 10 > Science Exam > Flashcards

Science Exam Flashcards

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1
Q

What is matter?

A

Anything that has mass and takes up space. Solid, liquid, or gas.

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2
Q

What is a mixture?

A

Mixtures retain their properties and can be seperated physically.

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3
Q

What does homogeneous mean?

A

Also known as solutions. Uniform distribution throughout all regions.

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4
Q

What does heterogeneous mean?

A

Not uniform distribution. Different properties in different regions.

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5
Q

What is a pure substance?

A

Constant composition. Only one type of particle.

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6
Q

When discussing matter, what is an element?

A

Composed of only one atom. Cannot be divided further by usual chemical or physical means.

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7
Q

What is a compound?

A

Individual components lose their identity. Can only be separated chemically.

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8
Q

What is a physical separation/change?

A

Does not change the composition of the matter; examples include changes of state (melting, evaporating, and freezing), filtration, etc.

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9
Q

What is a chemical separation/change?

A

The composition of the substance is altered; new substances are produced. Chemical changes are not usually easily reversed. Examples include burning, a metal reacting with an acid to produce hydrogen gas, etc.

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10
Q

At room temperature, what state are metals? Which element is the exception to this rule?

A

All are solid except mercury (liquid).

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11
Q

What describes metals’ appearance?

A

Shiny luster.

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12
Q

What describes metals’ conductivity?

A

Good conductors of heat and electricity.

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13
Q

What describes metals’ malleability and ductility?

A

Metals are malleable (hammered into thin sheets) and ductile (drawn into thin wires).

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14
Q

At room temperature, what state are non-metals? Which element is the exception to this rule?

A

May be solid, liquid, or gas. Not necessarily an exception, but bromine is the only liquid at room temperature.

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15
Q

What describes non-metals’ appearance?

A

No luster.

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16
Q

What describes non-metals’ conductivity?

A

Poor conductors of both heat and electricity.

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17
Q

What describes non-metals’ malleability and ductility?

A

Brittle and not ductile.

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18
Q

At room temperature, what state are metalloids?

A

Solid at room temperature.

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19
Q

What describes metalloids’ appearance?

A

Can be shiny or dull.

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20
Q

What describes metalloids’ conductivity?

A

May conduct electricity, but poor conductors of heat.

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21
Q

What describes metalloids’ malleability and ductility?

A

Brittle and not ductile.

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22
Q

What is an atom?

A

The basic unit of a chemical element.

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23
Q

In an atom, where are the protons and neutrons located?

A

In the center of the atom in the nucleus.

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24
Q

What is the atomic number? What does it represent?

A

The atomic number is the number on the bottom left corner. It represents the number of protons.

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25
Q

What is the mass number? What does it represent?

A

The mass number is the number in the top left corner. It represents the number of protons added to the number of neutrons.

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26
Q

What is the atomic mass?

A

The atomic mass is the number seen on the periodic table that is the average mass of all the isotopes of that element.

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27
Q

What are protons?

A

Part of an atom that is large and positive.

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28
Q

What are electrons?

A

Part of an atom that is small and negative.

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29
Q

What are neutrons?

A

Part of an atom that is large and have no charge.

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30
Q

Are atoms neutral or do they have a charge?

A

Atoms are neutral, meaning the amount of protons is equal to the amount of electrons.

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31
Q

What is an isotope?

A

Still the same element, but with a different number of neutrons and a different mass number.

32
Q

Where are electrons located?

A

In shells around the nucleus.

33
Q

What is the valence shell? What are valence electrons?

A

The outer shell is referred to as the valence shell. Valence electrons are the electrons in the valence shell.

34
Q

What is an ion?

A

A charged atom.

35
Q

What is a cation?

A

A positively charged ion. Known as electron donors.

36
Q

What is an anion?

A

A negatively charged ion. Known as electron receivers.

37
Q

What do Lewis Dot diagrams represent?

A

The number of valence electrons.

38
Q

How do ions form?

A

Since all elements want to have a perfect octet of electrons, they must either lose or receive electrons. This will give the atom a charge, making it an ion.

39
Q

What are ionic compounds?

A

Ionic compounds are bonds between a metal cation and a non-metal anion. The charges will equal zero. “Ide” is added to the end when naming

40
Q

What is a binary compound?

A

Two elements only.

41
Q

What are covalent compounds?

A

Covalent compounds are bonds between two or more non-metallic elements. Electrons are shared since both elements are looking to gain electrons.

42
Q

What type of compounds are molecules formed with?

A

Covalent compounds.

43
Q

What are the properties of ionic compounds?

A

Oppositely charged ions have a strong attraction. Tend to have high melting and boiling points because a lot of energy is needed to break the strong attraction. They conduct electricity when dissolved in water or are liquid. Melting or dissolving allows ions to move freely.

44
Q

What are the properties of covalent/molecular compounds?

A

The bonds within the molecule are strong but the force of attraction between the molecules is weak. They have low melting points because little energy is needed to break the forces of attraction between molecules. Relatively soft. Don’t conduct electricity in any state. Don’t conduct when dissolved in water because ions are not formed.

45
Q

What are electrolytes?

A

A substance that dissolves in water to produce a solution that conducts electricity. Ionic substances seem to be electrolytes while covalent/molecular substances seem to be non-electrolytes.

46
Q

What does exothermic mean?

A

Releases heat/energy.

47
Q

What does endothermic mean?

A

Gains heat/energy.

48
Q

What factors affect the speed of a reaction?

A
  • Presence of a catalyst
  • Concentration
  • Surface Area
  • Temperature
  • Pressure (with gases)
49
Q

What is a reactant?

A

Things that combine to form a new product.

50
Q

What is a product?

A

The result of two or more reactants.

51
Q

What is the law conservation of mass?

A

The law conservation of mass states that the total mass of the reacting substances is always equal to the total mass of the resulting substances. There is always the same number of atoms on both sides of the equation.

52
Q

What type of equation would this be?
X + Y –> XY

A

Synthesis/Combination, where two or more reactants combine to produce a new product.

53
Q

What type of equation would this be?
XY –> X + Y

A

Decomposition, where a compound breaks down into two or more compounds/elements.

54
Q

What type of equation would this be?
X + YZ –> YX + Z

A

Single Displacement/Replacement, where one element of a compound is replaced by a new element to form a new compound.

55
Q

What type of equation would this be?
WX + YZ –> YX + WZ

A

Double Displacement/Replacement, where the elements of two different compounds exchange places, forming two new compounds.

56
Q

What type of equation would this be?
CxHy + O2 –> CO2 + H2O

A

Combustion, because oxygen is combined with another compound and forms oxides. Produces carbon dioxide and water.

57
Q

What type of equation would this be?
CxHy +O2 –> CO2 + H2O + C + CO

A

Incomplete Combustion, where a hydrocarbon is burned in a poor supply of oxygen. Produces carbon dioxide, carbon monoxide, carbon (soot), and water.

58
Q

Define acids.

A

A chemical that produces hydrogen ions (H+) when dissolved in water (technically hydronium, H3O+).

59
Q

Give three examples of acids.

A

Lemon juice, vinegar, battery acid.

60
Q

What is the ionization equation for acids?

A

HCl (aq) → H+ (aq) + Cl- (aq)

61
Q

List the seven properties of acids.

A

Sour taste, many will burn skin, turns blue litmus paper red, reacts with metals and corrodes them, conducts electricity, pH < 7, produce hydrogen ions.

62
Q

Define bases.

A

A chemical that produces hydroxide ions (OH-) when dissolved in water.

63
Q

Give three examples of bases.

A

Soap, baking soda, antacids.

64
Q

What is the ionization equation for bases?

A

NaOH (aq) → Na+ (aq) + OH- (aq)

65
Q

List the seven properties of bases.

A

Bitter taste, slippery and many will burn skin, turns red litmus paper blue, no reaction with metals, conducts electricity, pH > 7, produces hydroxide ions

66
Q

What is the pH scale?

A

The pH scale measures how acidic or basic a solution is on a scale of 0-14.

67
Q

What is the pH of acids?

A

0-6

68
Q

What is considered a neutral pH?

A

7

69
Q

What is the pH of bases?

A

8-14

70
Q

How do you measure the pH of a solution?

A

Litmus paper (acids turn red, bases turn blue) or phenolphthalein (bases turn pink).

71
Q

Describe a neutralization reaction and provide an example using chemical formulas.

A

A neutralization reaction is a reaction between an acid plus a base resulting in water and a salt.

HCl + NaOH → salt + water
HCl + NaOH → NaCl + H2O
(all balanced)

72
Q

Provide a real-life example of neutralization.

A

Neutralization is used to maintain pools. Different chemicals, such as hypochlorous acid keep the pool clean, in turn lowering the pool’s pH. So, in order to balance it out, a base is added to achieve an ideal pH of 7.2-7.8.

73
Q

What is an ionic equation?

A

An ionic equation is a chemical equation in which the formulas of dissolved aqueous solutions are written as individual ions.

74
Q

What is acid rain and why is it harmful?

A

Acid rain is when carbon dioxide reacts with rainwater in the atmosphere and produces carbonic acid. Acid rain has a pH of below 5.5 and can be incredibly harmful to surrounding ecosystems. When the pH drops due to acid rain, many lakes end up losing different aquatic species and in a chain reaction, land animals don’t have enough food to eat.

75
Q

What is Arrhenius Theory?

A

This theory states that acids are substances that dissociate in water to yield electrically charged atoms or molecules, called ions, one of which is a hydrogen ion (H+), and that bases ionize in water to yield hydroxide ions (OH−).

Science 10 (2 decks)

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