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Science 9 (/10) > Unit B 3.0 > Flashcards

Unit B 3.0 Flashcards

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1
Q

What is ionization?

A

When an atom changes to an ion.

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2
Q

How does ionization occur?

A

When an atom gains or loses one or more electrons in order to become stable, or have their outermost energy level full.

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3
Q

If an atom has 1 electron in their outermost layer, will they gain 7 electrons or lose the 1?

A

Lose the 1, because atoms are lazy.

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4
Q

What is a positively charged atom called?

A

A cation.

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5
Q

What is a negatively charged atom called?

A

An anion.

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6
Q

How many electrons can an atom’s first energy level retain?

A

2 max.

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7
Q

How many electrons can every energy level except the first retain?

A

8 max.

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8
Q

If an atoms loses electrons it becomes

A

Positively charged.

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9
Q

If an atom gains electrons it becomes

A

Negatively charged.

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10
Q

Why does an atom become positively charged if it loses electrons?

A

Because electrons are negative charges.

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11
Q

All metals are __________ charged.

A

Positively.

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12
Q

All non-metals are __________ charged.

A

Negatively.

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13
Q

What is an ion charge?

A

The number or +/- sign that shows the number of electrons gained or lost.
Ex. Sc3+ — this atom lost 3 electrons, and therefore is 3+ positively charged.

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14
Q

What is a valence electron?

A

The electron that is taken away or added.

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15
Q

T/F: The electrons lost or gained are ALWAYS from the outermost energy level.

A

True.

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16
Q

How are groups of the periodic table based?

A

By ion charge.

Ex. All group 1s have +1, all group 2s have +2, etc.

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17
Q

Why are noble gases so unreactive?

A

Because they are already stable. They don’t want to gain or lose any electrons, so they don’t react.

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18
Q

What is an ionic bond?

A

Is the transfer of electrons between a metal and a non-metal.
Ex. Sodium and chlorine.

  • 1e -
  • 8e -
  • 2e -
    Na+
  • 7e -
  • 8e -
  • 2e -
    Cl-

Sodium will give their one electron to chlorine, so that way both of their outermost energy levels are full.
NaCl (s) — (ionic compound)

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19
Q

What is an ionic compound?

A

When a metal and a non-metal come together to create a neutrally-charged compound.
Ex. Aluminium (m) and fluorine (nm)

Al3+
Fl-

F- Al3+
F-
F-

AlF3 (s)

That way it’s neutral. You need 3 fluorides in order to be equivalent to 1 aluminium. It needs to be equivalent to be neutral.

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20
Q

T/F: All ionic compounds are not solid at room temperature.

A

False — they are.

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21
Q

T/F: if your metal is 2+ and your non-metal is 2-, they will cancel each other out and no subscript is needed.

A

True.

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22
Q

Metal + nonmetal =

Cation + anion =

A

Ionic compound.

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23
Q

What is the process for naming ionic compounds?

A
  1. Write the name of the metal ion first.
  2. Write the name of the non-metal ion last and change the ending to “ide”.
    Ex. KBr (s) — potassium bromide.
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24
Q

What is a univalent element?

A

An element with only 1 ion charge option.

Ex. Potassium

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25
Q

What is a multivalent element?

A 
An element with more than 1 ion charge option. 
Ex. Copper
Ex. lead (IV) oxide
nickel (III) sulfide 
copper (II) nitride
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26
Q

When should you use Roman numerals?

A

When the metal in an ionic compound is multivalent.

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27
Q

What is a polyatomic ion?

A

A group of atoms combined together that exist as a single unit with an overall electric charge.

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28
Q

Most polyatomic ions have a _______ charge.

A

Negative.

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29
Q

Where are polyatomic ions usually written in a formula?

A

Last.

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30
Q

What is the 1 exception to the rule that polyatomics behave as non-metals?

A

Ammonium.
NH +
…. 4
Behaves as a metal.

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31
Q

Why does ammonium behave as a metal?

A

Because it is positively charged.

32
Q

Do the endings change for polyatomic ions?

A

Nope.

33
Q

What is a dead giveaway that it’s a polyatomic ion?

A

The endings don’t change.

34
Q

What are the 3 polyatomic ions that have “ide” endings?

A
  1. Cyanide
  2. Hydroxide
  3. Hydrogen sulfide
35
Q

What is an effective way to find out what the ion charges of the atoms were before put into a compound name?

A

The reverse crisscross method.

36
Q

What is the thing that Mr. Whitehead said was STUPID IMPORTANT?

A

If there is only one subscript, you don’t need to add brackets. But if theres more than one, you NEED them.
Ex. NH42 / (NH4)2
First one says that there is 42 hydrogens. Second one says that there is 2 NH4s.

37
Q

Name 4 facts of ionic compounds.

A
  1. For every positive there is a negative.
  2. For every negative there is a positive.
  3. They’re all dependant.
  4. Metal w nonmetal.
38
Q

T/F: Ionic compounds form independent units.

A

False — they do not.

39
Q

Name 4 facts about molecules.

A
  1. Two or more non-metal atoms bonded together (all negatives!)
  2. Each molecule is independent of the next.
  3. They are NOT part of a lattice.
  4. NON-METAL W NON-METAL.
40
Q

What is a way to see if it’s an ionic or molecular compound?

A

Always look for the metal first. If there is a metal, it will always be ionic. If there’s no metal, just non-metals, it will always be molecular.

41
Q

What are molecular compounds?

A

Atoms linked together by sharing electrons.

42
Q

If non-metals always need to gain electrons to have a full outer shell, how do molecular compounds work?

A

The atoms share electrons.

43
Q

What is a covalent bond?

A

SHARING (not transferring) electrons from the outermost energy level.

44
Q

Draw 2 chlorine atoms being turned into 1 chlorine molecule.

A

Draw it.

45
Q

Go look in your camera role to see the examples of molecular compounds and covalent bonds.

A

Do it. Go. Now.

46
Q

What are monoatomic elements?

A

Elements that exist in nature as single atoms. Most elements are like this.

47
Q

What are diatomic elements?

A

Elements that exist in nature as pairs of atoms.

48
Q

How many diatomic elements are there?

A

7.

49
Q

How many polyatomic ELEMENTS are there?

A

2.

50
Q

How do you remember the diatomic elements?

A

I Bring Clay For Our New House.

51
Q

What are the diatomic elements?

A 
I2 (g): iodine
Br2 (l): bromine 
Cl2 (g): chlorine
F2 (g): fluorine
O2 (g): oxygen
N2 (g): nitrogen
H2 (g): hydrogen
52
Q

How do you remember the polyatomic elements?

A

And 4 Paving stones for 8 Steps.

53
Q

What are the polyatomic elements?

A

P4 (s): phosphorus

S8 (s): sulfur

54
Q

What is the FULL saying to memorize the polyatomic and diatomic elements?

A

I Bring Clay For Our New House, and 4 Paving stones for 8 Steps.

55
Q

What is the process for naming molecular compounds?

A
  1. Name the first element.
  2. Name the second element with an “ide” ending.
  3. Add the prefix indicating the number of atoms.
56
Q

What is the prefix for 1 atom?

A

Mono.

57
Q

What is the prefix for 2 atoms?

A

Di.

58
Q

What is the prefix for 3 atoms?

A

Tri.

59
Q

What is the prefix for 4 atoms?

A

Tetra.

60
Q

What is the prefix for 5 atoms?

A

Penta.

61
Q

What is the prefix for 6 atoms?

A

Hexa.

62
Q

What is the prefix for 7 atoms?

A

Hepta.

63
Q

What is the prefix for 8 atoms?

A

Octa.

64
Q

What is the prefix for 9 atoms?

A

Nona.

65
Q

What is the prefix for 10 atoms?

A

Deca.

66
Q

What happens if a compound has hydrogen present?

A

It has to go by a “common name”.

67
Q

What is the common name for H20?

A

Water.

68
Q

What is the common name for H2O2?

A

Hydrogen peroxide.

69
Q

What is the common name for NH3?

A

Ammonia.

70
Q

What is the common name for C3H8?

A

Propane.

71
Q

What is the common name for CH4?

A

Methane.

72
Q

What is the common name for CH3OH?

A

Methanol.

73
Q

What is the common name for C2H5OH?

A

Ethanol.

74
Q

What is the common name for C12O22H11?

A

Sucrose.

75
Q

What is the common name for C6H12O6?

A

Glucose.

Science 9 (/10) (3 decks)

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