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Chemistry > Semester 1 Final > Flashcards

Semester 1 Final Flashcards

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1
Q

5 examples of matter

A 
Calculator
Book
Desk
Shoe
Car
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2
Q

What is chemistry?

A

Chemistry is the study of matter and how it interacts, what its structure is and what properties it has

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3
Q

List the 3 states of matter –from least atomic connection to greatest atomic connection

A

Gasses – Liquids – Solids

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4
Q

What are the differences between Matter and Energy?

A

Matter has mass and volume in which it has atoms and can be weight, but energy cannot be weighed and has no atoms, mass and volume

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5
Q

Explain why gasses can be easily be compressed, but solids cannot.

A

Gasses can be easily compressed because the atoms are not bound together and are moving rapidly while solids cannot be compressed as much as gasses can because in solids, atoms are tightly packed together and they are moving very littl

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6
Q

List the 3 states of matter from most rapid atomic movement to least atomic movement.

A

Gasses – Liquids – Solids

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7
Q

List the three forms of energy discussed in class.

A

Electricity ~ Light ~ Heat

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8
Q

What is sublimation

A

When one state of matter gets skipped together

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9
Q

What is a phase change

A

A change in the state of matter of a substance

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10
Q

Explain why a pot of water will boil and turn to steam if it is heated.

A

A pot of after will boil and turn to steam when it is heated bc when you add more energy the atoms will move faster and faster. When the atoms move faster the bonds between atoms will break. The kinetic energy increases when you add energy. Atoms are like water molecules, when they are heated, they move faster and break bonds

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11
Q

Matter can be divided into 3 different categories, what are they?

A

Solids – Liquids – Gasses

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12
Q

What is a mixture

A

2 or more elements or compounds in the same place but not chemically combined

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13
Q

What are solids?

A

Solids have a definite shape, keep their shape and cannot be compressed

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14
Q

What are liquids?

A

Liquids shape changes to fit to its container and can be compressed a bit

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15
Q

What are gasses

A

Gasses have no true shape, expand to fill container. Can be compressed

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16
Q

Water will always be H2O. No matter where you find it it will be 2 hydrogens and 1 oxygen. If it isn’t then it isn’t water

A
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17
Q

Explain the difference between an element, compound and a mixture

A

An element is the simplest form of matter while a compound is made up of specific elements chemically combined. A mixture is two or more elements or compounds in the same place but not chemically combined.

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18
Q

List 3 characteristics of compounds

A

1) the elements of a compound are always found in the same ratio
2) individual elements properties disappear when the compound is formed
3) compounds can be broken down into simpler substances

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19
Q

What are two characteristics of all matter?

A

Has mass and has volume

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20
Q

Explain the difference between intensive and extensive properties

A

Intensive properties has the same in all sizes of a substance. Extensive properties depend on the amount of a sample

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21
Q

Describe how you know if a substance is going through a physical change

A
  • no new substance is formed
  • grinding
  • magnetizing iron
  • dissolving something
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22
Q

Describe how you know if a substance is going through a chemical change

A

A new substance is formed

  • a gas is produced
  • a precipitate forms
  • change in color
  • change in temperature
  • an odor is produced
  • energy is produced
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23
Q

The P-sublevel has how many orbitals

A

3

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24
Q

The d-sub level has how many orbitals

A

5

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25
Q

What is the overall charge of the nucleus

A

Positive

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26
Q

What is the overall charge of an atom

A

Neutral

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27
Q

What are protons

A

Protons have a positive charge and found in the nucleus

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28
Q

What are neutrons

A

Neutrons have no charge and are found in the nucleus

29
Q

What are electrons

A

Electrons have a negative charge and are found in the world electron cloud

30
Q

What are the 3 subatomic particles

A

Protons, neutrons, and electrons

31
Q

What is not an example of matter

A

Light

32
Q

Definition ionization energy

A

The energy needed to remove an electron

33
Q

Explain why the electronegativity changes when you move across the periodic table. >

A

It increases when you go across bc since you are gaining protons the pull on the nucleus will be greater. Therefore it will be easier to add electrons for it to become stable

34
Q

Definition atomic radius.

A

The distance from the nucleus to the valence electron

35
Q

Explain why the atomic radius changes when you go across the periodic table.

A

This is bc you are adding more protons when you move across therefore the pull on the nucleus is stronger making it closer to the nucleus

36
Q

Definition electronegativity

A

The tendency of an atom to gain an electron to become stable.

37
Q

Explain why the electronegativity changes when you go down the periodic table

A

The pull on the nucleus gets weaker and weaker as you go down further on the energy levels, therefore you are less likely to gain an electron because that bond is so weak since it is getting farther away from the nucleus

38
Q

Explain why the ionization energy changes when you go across the periodic table.

A

As you go across the protons are having a greater pull on the nucleus so it gets harder to remove an electron bc of this stronger pull

39
Q

As the atomic radius decreases, what happens to the ionization energy of those same elements?

A

The ionization energy increases.

40
Q

Ionic compounds are made up of:

A

Metals and nonmetals

41
Q

Covalent compounds are made up of:

A

Nonmetals and nonmetals

42
Q

Definition Polar Bond

A

They share electrons but not equally

43
Q

Definition nonpolar bond

A

They share electrons equally.

44
Q

Definition emulsifiers

A

Emulsifiers have both nonpolar and polar parts therefore they can dissolve almost anything

45
Q

4 properties of ionic compounds.

A

Hard, brittle
Form crystals
High melting and boiling point
Conduct electricity when dissolved in water

46
Q

What happens to an atom when its outer energy level gets filled?

A

It becomes stable

47
Q

Explain how a covalent bond forms and what happens to the valence electrons?

A

Form by nonmetals and nonmetals and the VE are being shared

48
Q

Definition bond length

A

The distance between 2 nuclei

49
Q

Definition bond energy

A

The energy needed to break a bond

50
Q

Explain how bond energy and bond length are related.

A

They are related because the longer the bond length, the less bond energy.

A triple bond is shorter therefore it requires lots of energy to break

51
Q

Explain how water dissolves ionic or polar covalent molecules.

A

Water is a slight positive and slight negative charge. Ionic and nonpolar has a charge. And the water is attracted to the molecules

52
Q

Explain how soap cleans oil.

A

Soap is an emulsifier. This means that it can dissolve almost anything in polar, ionic, and nonpolar.

53
Q

Definition emulsifier

A

Can dissolve almost anything with both polar and nonpolar parts

54
Q

What is the formula for an oxygen molecule?

A

O2

55
Q

Cation has a what type of charge?

A

Positive

56
Q

An anion has a what type of charge?

A

Negative

57
Q

Atoms form compounds so they can be…

A

More stable

58
Q

Ions tend to have the same electron configuration as noble gases

A

True

59
Q

Covalent bonds involve sharing electrons

A

True

60
Q

Ionic compounds have lower melting points.

A

False

61
Q

Nonpolar compounds are able to dissolve in liquid H2O

A

False

62
Q

How does ionic compounds use its valence electrons.

A

An ionic compound give and take electrons

63
Q

Which of the following is true when comparing two electrons which are in different shells of an atom

A

The electron in the higher numbered shell is further from the nucleus and is easier to remove

64
Q

The nucleons located in the nucleus of an atom are a combination of what?

A

Neutrons and protons

65
Q

The volume of space occupied by the electrons in comparison to the nucleus is?

A

About the same

66
Q

A compound is ?

A

A pure substance that is composer of 2 or more elements that are chemically combined.

67
Q

Definition heterogenous.

A

When you can see the different layers in a mixture.

68
Q

Definition Homogenous.

A

When you can see one solid layer ( 1 whole mixture)

Chemistry (4 decks)

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