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Chemistry > Chemical Bonding (topic 4) > Flashcards

Chemical Bonding (topic 4) Flashcards

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1
Q

What does BARF stand for?

A

Break a bond by Absorbing energy, Release energy when you Form a bond.

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2
Q

Which two atoms full shells only contain 2 valence electrons?

A

Hydrogen and Helium.

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3
Q

What rule do bonds between atoms work to achieve?

A

The octet rule.

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4
Q

What three things will atoms do with electrons to achieve a full outer shell?

A

Lose, gain, or share electrons.

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5
Q

You cannot have a single metallic bond. True or false?

A

True

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6
Q

In metallic bonds what happens to the electrons?

A

They move all around the metal, sea of electrons.

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7
Q

Examples of a metallic crystal.

A

Copper, silver, gold, brass

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8
Q

What metals are metallic substances made from?

A

Transition metals

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9
Q

Metallic substances have low melting and boiling points. True or false?

A

False

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10
Q

How do Ionic bonds form? What to they result in?

A

When a metal transfers own or more electrons to a non metal. This results in an ion.

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11
Q

Where do ion-ion electrostatic forces occur?

A

Ionic compounds.

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12
Q

Which structure is a part of ionic bonding?

A

Crystal lattice

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13
Q

Example of crystal lattice.

A

Salt crystals.

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14
Q

Ionic substances are conductors in a solid state. True or false?

A

False

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15
Q

Ionic substances are good conductors in solutions. True or false?

A

True

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16
Q

Do ionic substances have high melting and boiling points? If so why?

A

Yes, because of ion-ion forces.

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17
Q

Ionic substances dissolve is polar substances. True or false?

A

True (water is polar and salt is ionic)

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18
Q

How do covalent bonds form? What has to be the electronegativity difference?

A

Formed when to non metals share electrons. Electronegativity difference has to be less than 2.0.

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19
Q

What is a coordinate covalent bond ?

A

A covalent bond that forms when both electrons come from the same atom.

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20
Q

What is a non polar bond?

A

A bond with equal sharing of electrons due to atoms participating in the bond, having the same electronegativities.

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21
Q

What is a polar bond?

A

A polar bond is the unequal sharing of electrons due to the atoms in the bond, having a different electronegativity from each other.

22
Q

What does NASL stand for?

A

Needed
Available
Shared
Lone

23
Q

How do you use NASL?

A

Needed (2 for He+H, 8 for most others)

Available (add up valence electrons)

Shared (needed-available, this # divided by 2 tells you the number of bonds.)

Lone (Available-shared)

24
Q

How many bonds are made from one element being in group 14?

A

4

25
Q

How many bonds are made from one element being in group 15?

A

3

26
Q

How many bonds are made from one element being in group 16?

A

2

27
Q

How many bonds are made from one element being in group 17?

A

1

28
Q

How many bonds are made from one element being in group 18?

A

0

29
Q

What are the three ways to tell if a molecule is non polar?

A

1.Symmetrical
2. Hydrocarbon (made of just hydrogen and carbon)
3. One of the 7 diatomics

30
Q

What are the three ways to tell if a molecule is polar?

A
  1. Asymmetrical
  2. H-F, H-N, or H-O bonds are present
  3. Lone electrons pairs on the central atom.
31
Q

What does SNAP stand for?

A

Symmetrical means Nonpolar molecule, Asymmetrical means Polar molecule.

32
Q

Is H2O/water always polar or nonpolar?

A

Polar

33
Q

What is the structure of a molecule H2O/ water?

A

Bent

34
Q

What type of bond does dipole dipole intermolecular forces occur between?

A

Polar covalent

35
Q

In dipole dipole intermolecular forces the partial positive side of the molecules attracted to the partial negative side of a different molecule. True or false?

A

True

36
Q

Do intermolecular forces, connect atoms or molecules?

A

Molecules

37
Q

Where does hydrogen bonding occur?

A

Between molecules where a hydrogen is bonded to either an oxygen, nitrogen , or fluorine.

38
Q

In hydrogen bonding, does the hydrogen have the partially positive or the partially negative end?

A

Partially positive

39
Q

What type of intermolecular force occurs between all types of molecules?

A

LDF, london dispersion forces, Van Der Wall forces.

40
Q

What two types of intermolecular forces only occur between polar molecules?

A

Dipole dipole forces, and hydrogen bonding.

41
Q

What is the weakest type of intermolecular force?

A

LDF, london dispersion forces, Van Der Wall forces.

42
Q

The stronger, the intermolecular force, the lower, the melting and boiling points. True or false?

A

False

43
Q

What is a network solid?

A

A network solid is covalent bonds in a continuous network.

44
Q

Example of a network solid

A

Diamond, graphite, quartz

45
Q

What theory is used to name covalent molecules structure?

A

The VESPER theory

46
Q

What does VESPER in VESPER theory stand for?

A

Valence shell electron pair repulsion.

47
Q

Out of metallic, ionic, and covalent molecules which molecule is the only one that is soft?

A

Covalent

48
Q

What are the four types of structures in covalent molecules?

A

Linear, bent, trigonal pyramidal, and tetrahedral.

49
Q

Do covalent molecules have strong or weak intermolecular forces?

A

Weak

50
Q

What is the true definition of a chemical bond?

A

The forces that hold atoms together within a compound that’s goal is to have a full valance shell of electrons.

Chemistry (3 decks)

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