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Chemistry Honors > Chemistry Metallic, Ionic, & Covalent Bonding Test > Flashcards

Chemistry Metallic, Ionic, & Covalent Bonding Test Flashcards

1
Q

What kind of bonding is malleable and ductile

A

metallic

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2
Q

which forms lattices

A

metallic

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3
Q

which can conduct electrical and thermal energy

A

metallic

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4
Q

electrons form on attraction within a pool of electrons

A

metallic

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5
Q

strong absorbers and reflectors of light

A

metallic

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6
Q

electrons aren’t lost or shared, just helped together

A

metallic

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7
Q

formed between metals

A

metallic

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8
Q

C6H12O6

A

covalent

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9
Q

electrons are shared

A

covalent

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10
Q

results from a small difference in electronegativity

A

covalent

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11
Q

N2

A

covalent

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12
Q

boron trifluoride

A

covalent

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13
Q

can be solids, liquids, or gases

A

covalent

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14
Q

cannot conduct electricity when dissolved in water

A

covalent

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15
Q

compounds have lower melting and boiling points

A

covalent

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16
Q

chemical formula represents number of atoms in each individual molecule

A

covalent

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17
Q

formed between nonmetals

A

covalent

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18
Q

molecules

A

covalent

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19
Q

salts

A

ionic

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20
Q

NH4OH

A

ionic

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21
Q

chemical formula represents ration of ions in the crystal

A

ionic

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22
Q

electrons are transferred in the bond

A

ionic

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23
Q

can conduct electricity when dissolved in water

A

ionic

24
Q

form lattices

A

ionic

25
Q

form crystalline solids

A

ionic

26
Q

result from a large difference in electronegativity

A

ionic

27
Q

gold (I) oxide

A

ionic

28
Q

often formed between a metal and a nonmetal

A

ionic

29
Q

compounds have higher melting and boiling points

A

ionic

30
Q

Explain why most atoms form chemical bonds and
why some atoms don’t.

A

They form bonds to be stable with full outer energy levels
of electrons.
Noble gases don’t form chemical bonds because they are
already stable.

31
Q

Explain the difference between what a chemical
formula tells you about an ionic versus a covalent
compound.

A

In a covalent compound, the chemical formula tells you
exactly the number and types of atoms.
In an ionic compound, it represents the ratio of cations to
anions in the crystal lattice.

32
Q

Be able to explain what a chemical formula tells
you about a compound and predict properties of
the compound based on the bonds that hold it
together.

A

A chemical formula reveals the composition of a compound by specifying the types and ratios of atoms involved. The properties of the compound, including its melting point, conductivity, and reactivity, are largely determined by the nature of the bonds holding its atoms together, whether they are covalent, ionic, or metallic.

33
Q

Be able to identify a bond or a compound as ionic
or covalent based on a picture, description,
difference in electronegativity, or example.

A

You can identify a bond as ionic if it involves a transfer of electrons from one atom to another, typically between a metal and a nonmetal, resulting in the formation of ions with opposite charges. Covalent bonds, on the other hand, involve the sharing of electrons between atoms, usually between two nonmetals. For example, sodium chloride (NaCl) is ionic, formed between a metal (sodium) and a nonmetal (chlorine), whereas methane (CH4) is covalent, consisting of shared electrons between carbon and hydrogen atoms.

34
Q

Be able to use an element’s location on the
periodic table to predict its oxidation number and
bonding tendencies.

A

know oxidation numbers - cake

35
Q

List the number of atoms of each element in
the compounds below.
AlF3

A

Aluminum - 1
Fluorine - 3

36
Q

List the number of atoms of each element in
the compounds below.
K3P

A

Potassium - 3
Phosphorous - 1

37
Q

List the number of atoms of each element in
the compounds below.
Ca (ClO3)2`

A

Calcium - 1
Chlorine - 2
Oxygen - 6

38
Q

Explain the connection between electronegativity and the formation of the ionic bond.

A

The difference in electronegativity is so great that one atom takes an electrons from the other because it has such a greater attraction to them.

39
Q

Use an example of an ionic compound to explain the “rule of zero change”.

A

MgCl2 is one atom of magnesium with a 2+ charge, and two atoms of chlorine, each with a 1- charge.
1^(2+) + 2^(1-) = 2+ = 2- = 0

40
Q

Differentiate between binary ionic compounds, compounds with polyatomic ions, and binary molecular compounds

A

binary ionic - made of 2 elements that transfer electrons in an ionic bond
polyatomic - made of one (or more) covalently bonded charged groups of atoms that transfer electrons in an ionic bond
binary molecular - made of 2 elements that share electrons in a covalent bond

41
Q

give an example of a common compound and how the properties of the elements that make it up are different from that of the compound itself

A

NaCl = sodium chloride
Sodium on its own is extremely explosive when in contact with water
Chlorine on its own is extremely poisonous
Together they make table salt, which we can eat

41
Q

explain why it is necessary to include a Roman numeral when naming an ionic compound with a transition metal

A

you cannot determine the charge of a transition metal from the periodic table, so the Roman numeral is necessary to indicate the charge of the metal ion

42
Q

Name the following compounds:
Na2CO3
NH4C2H3O2
BaCl2
Mn(OH)2

A

sodium carbonate
ammonium acetate
barium chloride
manganese (ii) hydroxide

43
Q

Write the chemical formulas or the following compounds:
Magnesium fluoride
Calcium phosphate
Gold (II) carbonate
Lead (IV) sulfate

A

MgF2
Ca3(PO4)2
AuCO3
Pb(SO4)2

44
Q

Explain what makes a metallic bond different from
an ionic versus a covalent.

A

They are different from ionic because they do not lose their
valence electrons, instead they share.

They are different from covalent because they do not result
in a compound being formed.

45
Q

Explain why the “sea of e-” forms in metallic bonds
and why this makes them good electrical
conductors.

A

The “sea of e-” forms because metals like to form lattices,
but they are often bigger so their orbitals overlap. They
also have lower electronegativities so their attraction for
electrons in a bond is lower.

Because of this, the electrons are delocalized, making
them good at creating a flow of e- when conducting
electricity.

46
Q

Describe the unique properties that result from
metallic bonds.

A

Malleable (can be made into thin sheets)
Ductile (can be made into wires)
Can conduct electrical and thermal energy
Strong absorbers and reflectors of light

47
Q

Give an example of an alloy. Include what metals
make it up and how its structure aids in how the
alloy is used.

A

14K gold is part gold, part silver and copper (usually). This
alloy is stronger than gold on its own, making for more
durable jewelry.

48
Q

Explain the connection between electronegativity
and the formation of a covalent bond.

A

When the electronegativity difference is small, and thus
not big enough for one atom to take the electrons from the
other, the atoms share instead in a covalent bond.

49
Q

Differentiate between polar covalent and nonpolar
covalent bonds. Give an example of each.

A

Polar covalent are when electrons are unequally shared.

Ex. In H2O, the oxygen atom has a stronger attraction and pull on
the electrons than the hydrogen atoms, and thus the oxygen side
is a little more negative and the hydrogen side a little more
positive, creating poles.

Nonpolar covalent are when electrons are equally
shared, and the difference in electronegativity is 0.

Ex. In O2, electrons are equally shared between the 2 atoms.

50
Q

Differentiate between single, double, and triple
bonds.

A

Single = 2 shared e-

Double = 4 shared e-

Triple = 6 shared e-

51
Q

Explain how the VSEPR theory impacts how you
draw Lewis structures for molecular compounds.

A

VSEPR theory is the tendency for electron pairs to be as
far apart as possible from one another, and thus when you
draw Lewis structures for molecular compounds, you
should draw them in a way that spaces them out as much
as you can.

52
Q

Draw the Lewis structure for PCl3. Then write
its name.

A

Cl with 6 valence e- on both sides and bottom, surrounding P with 2 valence e- on top, and three dashes connected each Cl = Phosphorous trichloride

53
Q

Draw the Lewis structure for the hydroxide polyatomic ion

A

see review, slide 29

54
Q

Name the following compounds:
N2O3
SO2
N2S
B2H4

A

Dinitrogen trioxide
Sulfur dioxide
Dinitrogen monosulfide
Diboron tetrahydride

55
Q

Write the chemical formula for the following compounds:
Boron tribromide
Carbon tetrafluoride
Diphosphorous trisulfide
Nitrogen trihydride

A

BBr3
CF4
P2S3
NH3

Chemistry Honors (18 decks)

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