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Grade 10-11 SCIENCE > Chem Bond, Lewis, Naming > Flashcards

Chem Bond, Lewis, Naming Flashcards

1
Q

What is the process of ionic bonding?

A

Valence electrons are transferred between a metal and a non-metal to achieve the octet

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2
Q

What is a polyatomic ion?

A

A molecular compound that has an excess or deficit of electrons and thus has a charge.

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3
Q

Why do bonds bond together (other than octet, think charges)

A

They must combine with oppositely charged ions to achieve a neutral charge.

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4
Q

What is covalent bonding?

A

Electrons are shared between atoms because the electronegativity difference is not strong enough to completely pull valence electrons away.

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5
Q

What is indicated by arrows in polar covalent bonds?

A

The direction of electron pulling, pointing to the more electronegative atom.

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6
Q

Fill in the blank: The electronegativity difference for ionic bonding is greater than _______.

A

1.7

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7
Q

What must bonds do to ensure atoms achieve stability?

A

Give each atom 8 electrons.

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8
Q

Fill in the blank: The electronegativity difference for POLAR covalent bonding is between _______.

A

0.5 to 1.69

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9
Q

Fill in the blank: The electronegativity difference for NON-polar (or just covalent) bonding is below _______.

A

0.5

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10
Q

difference in electron sharing between ionic, polar covalent, and non-polar covalent bonds

A

i: electrons are transferred, pc: partially shared/unequal, n-pc: shared equally

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11
Q

define single, double, and triple bond

A

single bond: results from covalent bond sharing ONE pair of electrons (H and H)

double bond: sharing TWO pairs (C and O)

triple bond: sharing THREE pairs (N and N)

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12
Q

define bonding pair and lone pair

A

bonding: a pair pf electrons that is shared between 2 atoms

lone: a pair of electrons that is NOT shared

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13
Q

Where do H and F go in a Lewis structure

A

ALWAYS at the end

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14
Q

which goes in the center? most electropositive or most electronegative?

A

most electropositive

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15
Q

What makes a lewis structure bent?

A

if there’s a lone pair on the CENTRAL atom, doesn’t matter the #, it will make the structure bend (repulsion)

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16
Q

what is the math letters and meaning for doing Lewis structures

A

V = valence
T = total
S = shared bonds
NB = non-bonding pair

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17
Q

explain the written math steps for Lewis structure (NF3)

A

ex. NF3
1. (V) det total valence electrons in all atoms at start [N: 1(5) / F: 3(7)] = 26

  1. (T) det total # of electrons needed to reach octet
    [N: 1(8) / F: 3(8)] = 32
  2. (S) T-V= Answer /2
    [32 - 26 = 6 / 2 = 3 bonding pairs]
  3. (NB) V-S= Answer / 2
    [26 - 6 = 20 / 2 = 10 lone pairs]
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18
Q

Which 2 elements have a special octet total # and what is the number?

A

S = 12, P = 10

19
Q

Between 2 compounds, how do you know which one has a greater intermolecular force?

A
  1. identify what intermolecular force each uses, may be able to determine from that
  2. both LDF? check molecular weight. The larger one is your answer.
  3. for dipole-dipole, its the one with the higher EN difference
20
Q

What are the types of intermolecular forces? (4)

A

ion-dipole, dipole-dipole, hydrogen bond, London dispersion force or Van der Waals forces

21
Q

What is a hydrogen bond? example?

A

A dipole bond between H and O, F, or N. It is the strongest type of intermolecular bond. H2O, HF, strong because high electronegativity difference

22
Q

types of intramolecular bonds

A

ionic , polar covalent, or covalent!

23
Q

Describe London Dispersion Forces?

A

Weak forces present in non-polar molecules that strengthen as the size of the molecule increases, and disperse very quickly. Its basically imbalance in the electron cloud and all bonds do this atleast slightly.

24
Q

Fill in the blank: Solubility follows the principle of _______.

A

Like Dissolves Like.

25
Q

How do ionic compounds behave in water?

A

They mix with charged and polar substances, ions dissociate, and the solution can conduct electricity.

26
Q

How do covalent compounds behave in water?

A

They mix with charged and polar substances but do not break apart into ions, so the solution does not conduct electricity.

27
Q

What affects the melting and boiling points of molecular compounds?

A

The strength of intermolecular forces: H-bonding > dipole-dipole > London Dispersion.

28
Q

Why do ionic compounds have higher melting and boiling points than molecular compounds?

A

Due to their strong crystal lattice structure.

29
Q

What is chemical nomenclature?

A

A system of names used in chemistry, approved by IUPAC

30
Q

What defines multivalent metals?

A

Metals that can have more than one valence or charge

31
Q

What does the suffix ‘-ous’ signify?

A

The lower of the two ion charges

32
Q

What does the suffix ‘-ic’ signify?

A

The higher of the two ion charges

33
Q

What is the formula for copper(II) sulfate pentahydrate?

A

CuSO4•5 H2O

34
Q

What is the classical name for HCl(aq)?

A

Hydrochloric acid

35
Q

How are non-polyatomic acids named?

A

Add prefix hydro- with the stem of the element, and ending -ic

36
Q

What is an oxyacid?

A

An acid containing oxygen, hydrogen, and a third element

37
Q

What does the prefix thio- indicate?

A

An oxygen atom in the compound has been replaced by a sulfur atom

38
Q

What is the formula for sulfate?

A

SO4

39
Q

What is the formula for thiosulfate?

A

S2O3

40
Q

What is the formula for thiosulphite?

A

S2O2

41
Q

what does IUPAC stand for

A

International Union of Pure and Applied Chemistry

42
Q

list the suffix and prefix combo in order of levels of ions

A

per-ate
ate
ite
hypo-ite

43
Q

how do you write the formula of an acid?

A

add as many H to the compound to take off the entire charge (neutral)

44
Q

How are polyatomic acids named?

A

the stem of the polyatomic ion, and ending in ic if the ion starts and/or ends with per-ate, and ous if it starts and/or ends with hypo-ite

Grade 10-11 SCIENCE (10 decks)

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