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Chemistry--SCH3U > Unit 1-- Matter, chemical trends, & chemical bonding > Flashcards

Unit 1-- Matter, chemical trends, & chemical bonding Flashcards

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1
Q

What is all matter composed of?

A

Atoms

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2
Q

What are the 3 sub-atomic particles?

A

Protons, Neutrons, and Electrons

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3
Q

How are ions formed?

A

When an atom gains or loses an electron, it becomes an ion and is no longer neutrally charged

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4
Q

ions

A

Charged atoms

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5
Q

Define ISOELECTRONIC

A

Atoms/Ions that have the same number of electrons

same number of valence electrons.

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6
Q

ANION

A

An atom that gains electrons becomes NEGATIVELY charged

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7
Q

CATION

A

An atom that loses electrons and becomes POSITIVELY charged

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8
Q

Two or more forms of the same element that have the same number of protons but a different number of neutrons

A

ISOTOPES

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9
Q

Can differ in mass and there can be heavy and light forms of an element

A

ISOTOPES

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10
Q

ELECTRON PAIRS

A

Two electrons interact in a unique way, allowing them to be situated close to each other

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11
Q

UNPAIRED ELECTRONS

A

Electrons that are in an unfilled outer shell and do not have pairs.
They are more likely to participate in atom bonds

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12
Q

ATOMIC MASS UNIT

A

U
a measure of its atomic mass.
it is one-twelfth of the carbon-12 atom

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13
Q

BETA PARTICLE

A

High energy particles that are negatively charged, and are ejected from the nucleus when the nucleus is unstable and unbalanced

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14
Q

AVERAGE ATOMIC MASS

A

The average of the masses of all the elements isotopes

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15
Q

How are BETA particles formed?

A

emitted from an atom’s nucleus during radioactive decay.

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16
Q

RELATIVE ATOMIC MASSES

A

The weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12

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17
Q

STRONG NUCLEAR FORCE

A

the force that holds protons and neutrons together.

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18
Q

RADIOSOTOPES

A

Isotopes with unstable nuclei that decay into different, often more stable isotopes

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19
Q

ISOTOPIC ABUNDANCE

A

The percentage of atoms with a specific atomic mass found in an element

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20
Q

How many isotopes is CARBON made of

A

2!

Carbon-12 & Carbon-13

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21
Q

What holds the nucleus ( protons and neutrons) together

A

STRONG NUCLEAR FORCE

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22
Q

ENERGY LEVELS

A

fixed distances from the nucleus of an atom where electrons may be found

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23
Q

BOHR MODEL

A

consists of a small, dense nucleus surrounded by orbiting electrons.

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24
Q

LEWIS DOT DIAGRAMS

A

use dots to represent valence electrons around an atomic symbol.

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25
Q

OUTERMOST ELECTRONS

A

VALENCE ELECTRONS

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26
Q

1st energy level

A

Holds 2 electrons

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27
Q

2nd energy level

A

Holds 8 electrons

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28
Q

3rd energy level

A

Holds 8 electrons

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29
Q

OCTET RULE

A

This tendency to gain or lose electrons
is called the

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30
Q

PERIODIC LAW

A

A statement that describes the repeating nature of the properties of the elements

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31
Q

PERIOD

A

Rows on the periodic table of elements

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32
Q

GROUP

A

Columns on the periodic table of elements

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33
Q

METALLOIDS

A

Along both sides of the staircases and demonstrate both metal and non-metal properties

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34
Q

HALOGENS

A

-Many are are liquids or gases
- Very poisonous
- Reactivity increases UP the group

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35
Q

NOBLE GASES( INERT GASES)

A

– All are gases
- Do not react with anything

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36
Q

ALKALINE EARTH METALS

A
  • Solids
    -React with metals less dramatically than less active metals
    -Reactivity increases DOWN the group
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37
Q

ALKALI METALS ( ACTIVE METALS)

A
  • Solids
  • Very reactive and reacts violently with water
  • Reactivity increases DOWN the group
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38
Q

When elements are arranged by atomic number, their chemical and physical properties recur periodically

A

PERIOD LAW

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39
Q

ATOMIC RADIUS

A

the total distance from the nucleus of an atom to the outermost orbital of its electron.

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40
Q

TRANSITION METALS

A

Thier electron configuration is more complex than main-group elements
They make the periodic table 18 columns wide

41
Q

SHIELDING..

A

the outer electrons are shielded and thus have less grip on the nucleus.

42
Q

*ATOMIC SIZE/ RADIUS

A

As you go down each GROUP in the periodic table, the size of an atom INCREASES

As you go across each group on the table the size decreases

43
Q

**ATOMIC SIZE/ RADIUS

A

As you go ACROSS A PERIOD, the size of an atom DECREASES

44
Q

IONIZATION ENERGY

A

The energy that is required to REMOVE an electron

45
Q

Tends to DECREASE down a group

A

IONIZATION ENERGY

46
Q

Tends to INCREASE across a period

A

IONIZATION ENERGY

47
Q

ELECTRON AFFINITY

A

The energy associated with the ADDITION of an electron to a neutral atom

48
Q

Tends to DECREASE down a group and increase across a period

A

ELECTRON AFFINITY

49
Q

ELECTRONEGATIVITY

A

The measure of an atom’s ability to attract electrons in a chemical bond

50
Q

Electronegativity INCREASES up a group across a period

A

Yes :)

51
Q

EFFECTIVE NUCLEAR CHARGE

A

The apparent nuclear charge, as experienced by the outermost electrons of an atom, as a result, shielding occurs

52
Q

ATOMIC RADIUS

A

The distance from the centre of an atom to the boundary within the electrons

53
Q

PERIODIC LAW

A

When elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties.

54
Q

Metals vs Non-metals

A

METALS
-Left side of the staircase
-Most are solid and shiny
-Good conductors of heat and electricity
-tend to LOSE electrons and become positive ions

NON-METALS
-On the right side of the staircase
-Many are liquids and gases
-poor conductors (good insulators) of heat and electricity
Tend to gain electrons and become negative ions

55
Q

IONIC BONDING

A

In an IONIC BOND electrons are transferred from a metal to a NON-metal

56
Q

COVALENT BONDING

A

A COVALENT BOND is formed when a pair of electrons are paired between 2 or more non-metals

57
Q

ELECTRONEGATIVITY (EN)

A

The measure of an atom’s ability to attract electrons in a chemical bond

it increases up a group and across a period

58
Q

Only non-metals form covalent bonds

A

:)

59
Q

What do covalent bonds form?

A

MOLECULES!

60
Q

IONIC COMPOUNDS VS MOLECULAR COMPOUNDS

A

IONIC COMPOUNDS
-Crystalline Solids
-High melting points
-conduct electricity
-most have high solubility in water

MOLECULAR COMPOUNDS
-Solids, Liquids, gases
-Low melting point
-Does not conduct electricity
Low solubility in water

61
Q

^EN= >1.7

A

IONIC

62
Q

^EN between 0.5-1.7

A

POLAR COVALENT

63
Q

^EN between 0-0.4

A

SLIGHTLY POLAR COVALENT

64
Q

^EN=0

A

NON POLAR COVALENT ( PURE COVALENT)

65
Q

SINGLE BOND

A

A covalent bond that results from atoms sharing one pair of electrons

66
Q

DOUBLE BOND

A

A covalent bond where atoms share two pairs of electrons

67
Q

TRIPLE BOND

A

A covalent bond where atoms share three pairs of electrons

68
Q

LONE PAIR

A

A pair of electrons that’s not part of a covalent bond

69
Q

LEWIS STRUCTURE

A

a very simplified representation of the valence shell electrons in a molecule

Lewis dot diagram

70
Q

OCTET RULE

A

When bonds form between atoms, the atoms gain or lose electrons or share electrons, that way they create a filled outer shell containing 8 electrons

71
Q

When two atoms form a bond…

A

each atom attracts the other atom’s electron as well as its own

72
Q

How to calculate ATOMIC MASS

A

Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances.

73
Q

How to calculate ISOTOPIC ABUNDANCE

A

Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances

74
Q

Note

A

Electron negativity increases as the size of the atom decreases

75
Q

Binary Compound

A

An ionic compound that consists of only two ( bi) elements

76
Q

Naming Ionic Compounds

A

Metal comes first and non-metal gas comes second but the ending is changed to “ide”

77
Q

Transition Metals

A

Stock system– Roman numerals are used to indicate ionic charge

“ic” and “ous”– endings- only applied to some transition metals that only have 2 possible ionic charges

78
Q

BINARY IONIC COMPOUND

A

contains an ion that is a metal (cation) and an ion that is a nonmetal (anion).

79
Q

ALKALI

A

A base that is soluble in water

80
Q

OXOACIDS

A

An acid composed of hydrogen, oxygen, and atoms of at least one other element

81
Q

STRUCTURAL FORMULA

A

A diagram that has the chemical symbols connected by lines to show the connections among atoms in a chemical compound

82
Q

NAMES/STRUCTURES FOR MOLECULAR COMPOUNDS

A
  1. MONO
  2. DI
  3. TRI
  4. TETRA
  5. PENTA
  6. HEXA
  7. HEPTA
  8. OCTA
  9. NONA
  10. DECA

EG.
S,F6–> sulfur HEXAfluoride

83
Q

POLYATOMIC IONS/ RADICALS

A

Ions that are composed of more than one element are called polyatomic ions

84
Q

ACIDS VS BASES

A

ACIDS
- Taste sour
-Conducts electricity in aqueous solutions
-turns litmus paper RED
-Feels wet
-Reacts with some metals to form H2 (g)
-Reacts with carbonates to form CO2

BASES
-Taste Bitter
-Conducts electricity in aqueous solutions
Turns litmus paper BLUE
-Feels slippery
-Does not react with metals
-Does not react with Carbonates

85
Q

1 O (oxygen) more–SO5^-2

A

PERsulfate

86
Q

MOST COMMON –> SO4^-2

A

SULFATE

87
Q

1 O less –> SO3^-2

A

sulfIITE

88
Q

2 O Less –> SO2^-2

A

HYPOsulfITE

89
Q

ACIDS

A

ACIDS
- Taste sour
-Conducts electricity in aqueous solutions
-turns litmus paper RED
-Feels wet
-Reacts with some metals to form H2 (g)
-Reacts with carbonates to form CO2

90
Q

BASES

A

BASES
-Taste Bitter
-Conducts electricity in aqueous solutions
Turns litmus paper BLUE
-Feels slippery
-Does not react with metals
-Does not react with Carbonates

91
Q

ACID & BASE NOMENCLATURE
BASES

A

Bases are IONIC COMPOUNDS
eg.

KOH - Potassium hydroxide
Na OH - Sodium hydroxide

92
Q

BASES

A

Ionic Compounds

eg. KOH –potassium hydroxide

93
Q

TWO TYPES OF ACIDS

A

Binary acids & Oxyacids

94
Q
  1. BINARY ACIDS
A

HX where X is the nonmetal ( usually a halogen)

you must state the HYDRO first, and then end the nonmetal’s name with an “ic” ending and the word “acid”

eg.
HF– Hydrofluoric acid
HCl– Hydrochloric acid

95
Q

ORDER OF BINARY ACIDS

A

HX ( X is nonmetal)
1. state HYDRO
2. end the nonmetal with “ic”
3. end with the word “acid”

96
Q
  1. OXYACIDS
A
  • Contain H and a polyatomic ion ( that contains o)
  • Use the beginning of the polyatomic ion name
    add an “ic” ending
  • Add the word “acid”

eg. HNO3– Nitric acid
Sulfuric acid –> H2,SO4

97
Q
  • Contain H and a polyatomic ion ( that contains o)
  • Use the beginning of the polyatomic ion name
    -add an “ic” ending
  • Add the word “acid”
A

OXYACIDS

98
Q

Different Oxyacids can be found by changing the number of oxygen atoms contained in the polyatomic ion

A

1 O (oxygen) more– H2 SO5 – PERsulfuric acid
Most common– H2 S04 – sulfuric acid
1 O less– H2 SO3 – H2 SO3 –sulfurOUS acid
2 O less– H2 SO2 – HYPOsulfurOUS acid

Chemistry--SCH3U (4 decks)

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