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Chemistry > Bonding > Flashcards

Bonding Flashcards

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0
Q

What is a cation?

A

A cation is a metallic ion.

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1
Q

Na and Cl bond so well because…

A

Na is a metal and its ion is Na+. Cl is a nonmetal and its ion is Cl-. Na has the electron chlorine wants, so they share it to create a noble gas configuration. This is a salt.

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2
Q

What is an anion?

A

An anion is a nonmetallic ion.

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3
Q

Why are ions formed?

A

Ions are formed so atoms can create a noble gas configuration.

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4
Q

What is the Lewis Dot Diagram for hydrogen?

A

.

H

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5
Q

What is the Lewis Dot Diagram for NaCl?

A

..
[Na]+[:Cl:]-
..
The plus sign next to Na and the negative sign next to Cl represent the charge, not addition and subtraction

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6
Q

How many lithium ions would be needed to neutralize the charge of an oxygen ion?

A

2 would be needed. A lithium ion has a charge of +1 and an oxygen ion has a charge of -2. You would need 2 lithium ions to create a charge of +2, which would neutralize the charge of -2.

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7
Q

Ionic compounds have a difference greater than or equal to

A

1.7

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8
Q

MgCl can be expressed as

2

A

Magnesium chloride

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9
Q

Iron (II) varies from iron (III) in what way?

A

The Roman numerals indicate the charge of the ion.

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10
Q

Iron (III) oxide can be expressed as

A

Fe O

2 3

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11
Q

Endothermic means

A

Absorbing heat (examples: melting, boiling)

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12
Q

Exothermic means

A

Releasing heat (example: combustion, aka fire)

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13
Q

What is an ion?

A

An ion is an atom that has lost or gained electrons to achieve a noble gas configuration.

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14
Q

What is a compound?

A

2 or more DIFFERENT atoms that are chemically combined in definite proportions.
NaCl - compound
Ammonium phosphate - compound
Ozone (O3) - not a compound

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15
Q

Are the radii of cations greater or smaller than that of the neutral state?

A

Smaller

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16
Q

Are the radii of anions smaller of larger than that of the neutral state?

A

Large

17
Q

What are characteristics (both quantitative and qualitative) of ionic bonds?

A

High melting points, good conductivity in liquids (usually when dissolved in water), hard texture, and an electronegativity difference of 1.7 or greater.

18
Q

What creates conductivity?

A

Mobile electron

19
Q

What are the diatomics?

A

HOFBrINCl

Hydrogen, Oxygen, Flourine, Bromine, Iodine, Nitrogen, and Chlorine

20
Q

Diatomics form what kind of bond?

A

Nonpolar covalent

21
Q

What types of elements form covalent bonds? Ionic bonds?

A

Ionic bonds are formed by metals and nonmetals. Covalent bonds are formed by nonmetals.

22
Q

True or false:

In a covalent bond, attraction is less than repulsion.

A

False.

In a covalent bond, attraction between atoms is greater than repulsion.

23
Q

What is a common goal of ionic and covalent bonds?

A

A common goal is to form octets.

24
Q

What are the characteristics of covalent bonds?

A

Soft, poor conductors of electricity, low boiling and melting point, not very soluble, and tend to be flammable.

25
Q

Draw a Lewis Dot Diagram for methane.

A 
H
               |
       H— C — H
               |
              H
26
Q

Double and triple bonds are much __________ and __________ than single bonds.

A

Stronger and shorter

27
Q

Draw a Lewis Dot Structure diagram for dinitrogen monoxide with a charge of -1.

A

.. .. .. -1
[:O=N—O:]
..

28
Q

What are the prefixes for numbers 1-10?

A

Mono (only for oxygen), di, tri, tetra, penta, hexa, hepta, octa, nona, deca

29
Q

What are the 5 formulas to remember?

A 
Water - H2O
Ammonia - NH3 (not ammonium)
Methane - CH4
Hydrogen peroxide - H2O2
Glucose - C6H12O6
30
Q

What is used when molecular compounds have multiple Lewis Dot Diagrams?

A

Calculate formal charge for each atom in the molecular compound. Look for the most stable.
Formal charge = valence electrons - (number of bonds + number of lone electrons)

31
Q

What is the difference between resonance and a hybrid Lewis Dot Diagram?

A

Resonance shows all different combinations concerning location of bonds and lone electrons. A hybrid doesn’t show lone electrons and shows a dotted line next to a bond.

32
Q

What are the exceptions to the octet rule?

A

Hydrogen, odd number of valence electrons, atoms with fewer than 8 valence electrons in a full valence shell, and expanded octets (atoms with more than 8 valence electrons, occurs only in elements in a Period 3 and above. An example is sulphur hexafluoride)

33
Q

What is the definition of a covalent bond?

A

A covalent bond is a bond between atoms that is formed by the sharing of electrons rather than the transfer of electrons.

34
Q

What are the electronegativity difference ranges for bonds?

A

Ionic has a range of 1.7-4.0
Polar has a range of 0.4-1.7
Nonpolar has a range of 0.0-0.4

35
Q

What is the difference between polar and nonpolar bonds?

A

Nonpolar covalent bonds have an equal attraction for shared electrons (example: diatomics) whereas polar covalent bonds have an unequal attraction for shared electrons (example: hydrogen chloride)

36
Q

True or false: In nonpolar molecules, dipoles pull electrons slightly towards one atom and slightly away from another, creating a slightly negative and slightly positive side.

A

False. This occurs in polar molecules.

37
Q

What kind of molecule is carbon tetrachloride? What kinds of bonds does it have?

A 
Polar bonds
Nonpolar molecule (look at symmetry)
38
Q

True or false: Any diatomic with a polar bond is a polar molecule. Example: Carbon monoxide

A

True

39
Q

Is it true to conclude that diatomic molecules that have nonpolar bonds are nonpolar molecules?
Examples: chlorine, oxygen

A

True

40
Q

Three or more atoms are polar unless:

A

The central atom has no lone pairs and is surrounded by atoms of one element.

Chemistry (4 decks)

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