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Gen Chem > Q3 > Flashcards

Q3 Flashcards

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1
Q

Kinetic Molecular Theory

A

all matters are made up of atoms and molecules that are always moving.

These particles hold kinetic energy and move around in random directions.

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2
Q

force that hold atoms together in a metallic substance.

A

Metallic bond

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3
Q

formed between two or more atoms by transfer of one or more electrons between atoms
- electrons are transferred

A

Ionic bond

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4
Q

particle with unequal number of protons and electrons

A

Ions

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5
Q

negative ions

A

Anions

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6
Q

postively charged

A

Cations

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7
Q

consists of the mutual sharing of one or more pairs of electrons between two atoms.

A

Covalent bond

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8
Q

2 types of covalent bonds

A

Polar covalent, non-polar covalent bonds

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9
Q

forces within ionic compounds and simply the attraction between negative and positive ions (anions and cations attract).

A

Ion-ion forces

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10
Q

attraction between two polar molecules

A

Dipole-dipole

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11
Q

is a principle/idea/model that is used to explain the behavior, movement of particles/molecules for every states of matter from a microscopic point of view.

A

KMT

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12
Q

This theory explains the states of matter, and is based on the idea that matter is composed of tiny particles that are always in motion. This theory helps explain observable properties and behaviors of solids, liquids, and gases

A

KMT

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13
Q

KMT states that:

A
  1. Matter is made up of particles that are constantly moving.
  2. All particles have energy, but the energy varies depending on the temperature the sample of matter is in.
  3. The temperature of a substance is a measure of the average kinetic energy of the particles.
  4. A change in phase may occur when the energy of the particles is changed.
  5. There are spaces between particles of matter. The average amount of empty space between molecules gets progressively larger as a sample of matter moves from the solid to the liquid and gas phases.
  6. There are attractive forces between atoms/molecules, and these become stronger as the particles move closer together. These attractive forces are called intermolecular forces.
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14
Q

region of space where all physical and chemical properties are uniform.

A

Phase

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15
Q

Liquids and solids

A

Condensed phase

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16
Q

A state change of any material due to temperature or pressure change is a phase transition. It is a physical change (or reaction).

A

Phase transition

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17
Q

solids whose particles are arranged in regular geometric patterns.

  • Rigid and incompressible
  • Sharp melting point
A

Crystalline solids

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18
Q

have fixed shape and volume but their particles are not arranged in a regular geometric pattern.

  • also referred to as “supercooled” liquids because these solids appear to have been cooled at very low temperatures and their viscosities are very high.
  • No definite heat of fusion
A

Amorphous solid

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19
Q

Glass is an example of

A

Amorphous solid

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20
Q

lattice points are occupied by molecules, molecules are packed closely as their size and shape allow , IMF may be LDF in the case of non-polar crystals, dipole-dipole for polar crystals, and some cases such as ice have hydrogen bonding.

A

Molecular solids

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21
Q

the constitution particles are ions
- formed by the arrangement of cations and anions by strong coulombic forces
- atoms are held together by electrostatic force
- held firmly and no large space for the ions to move around

A

Ionic solids

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22
Q

positive metal ions in a sea of delocalized electrons. These electrons are evenly spread out throughout the crystal
- held together by electrostatic force between cations and delocalized electrons (metallic bonds)

A

Metallic solids

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23
Q

a covalent network crystal consists of atoms at the lattice points of the crystal

A

Covalent solids

24
Q

is a graph that relates pressure and temperature to the state of matter.
The diagram can help us identify what is the state of a substance at a given temperature and pressure.

A

Phase diagram

25
Q

is the point where at a certain pressure and temperature at equilibrium all three phases of a substance co-exist.

A

Triple point

26
Q

is a point where temperature and pressure at which gas and liquid merge together to form a supercritical fluid.

A

Critical point

27
Q

is any substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not exist.

A

Supercritical fluid

28
Q

is where a substance is impossible to liquefy no matter how you increase or compress the substance.

A

Critical temperature

29
Q

is a plot where it shows how the addition of heat (x-variable) can affect the temperature change (y-variable) and phase change of a substance.

A

Heating curve

30
Q

Types of Solutions

A

Saturated
Unsaturated
Super saturated

31
Q

Solvent holds as much solute as is possible at that temperature.

A

Saturated

32
Q

Less than the maximum amount of solute for that temperature is dissolved in the solvent.

A

Unsaturated

33
Q

Solvent holds more solute than is normally possible at that temperature.

A

Super saturated

34
Q

These solutions are unstable; crystallization can usually be stimulated by adding a “seed crystal” or scratching the side of the flask.

A

Super saturated

35
Q

refers to the amount of solute present in a given quantity of solvent or solution.

A

Concentration of solution

36
Q

if less than or equal to 0.1g of solute dissolves in 100g of solvent

A

Insoluble solute

37
Q
  • if the amount of solute that dissolves in 100g of solvent is greater than 0.1g but less than 10g.
A

Slightly soluble solute

38
Q

if less than or equal to 0.1g of solute dissolves in 100g of solvent

A

Insoluble solute

39
Q

if the amount of solute that dissolves in 100g of solvent is greater than or equal to 10g.

A

A soluble solute

40
Q

What type of IMF must be predominantly overcome when a molecule of ammonia (NH3) escapes from liquid ammonia?

A

H-bond

41
Q

Consider a list of liquids that have only London Forces as intermolecular interactions. What happens to the boiling point, vapour pressure and surface tension, respectively, as the molecular weight of these liquids increases?
Increases, decreases, increases Increases, decreases, decreases
Decreases, increases, decreases Decreases, increases, increase

A

Increase, decreases, increases

42
Q

Tendency of molecules of the same kind to stick one another.

A

Cohesion

43
Q

Which of the following changes would increase the vapor pressure of a liquid?
A decrease in temperature
A decrease in the intermolecular forces in the liquid.
An increase in the size of the open vessel containing the liquid.

A

A decrease in the intermolecular forces in the liquid.

44
Q

Humans have physiologically adapted to sweat if the body temperature rises past ideal levels. The ability to do so helps cool the body down. Water’s ___________ allows us to maintain homeostasis – body regulating itself to maintain balance like body temperature – and survive as we are today.

A

High specific heat

45
Q

Water molecules bond in a crystalline form as the temperature of water drops. The molecules rearrange to form hexagonal ring. This creates more space between molecules and expansion of water molecules. What characteristic of water does this change describe?

A

Density

46
Q

H2S

A

Hydrosulfuric acid or Hyrogen Sulfide

47
Q

Mg3N2

A

Magnesium nitride

48
Q

NaHCO3

A

Sodium Bicarbonate

49
Q

Cu3(PO4)2

A

Copper (II) phosphate

50
Q

Cl2O7

A

Dichlorine heptoxide

51
Q
  1. Capillary Action is caused by adhesion and cohesion forces.
  2. CO2 has higher vapor pressure than NaCl.
  3. Liquid water has a specific heat of 4.18 J/g-Co and iron has 0.45 J/g-Co, this data shows that liquid water gets
    hotter faster than the iron.
  4. As temperature gets higher, average kinetic energy of molecules increases.
  5. Liquids and gases are the phases we considered as fluids.
  6. According to KMT, all particles are always in constant motion.
  7. The stronger the adhesive force, surface tension also gets stronger.
  8. Fluids with high fluidity flows slowly.
  9. As the average kinetic energy of your molecules increases, molecules tend to move away from each other.
  10. KCl which is a salt is a polar molecule and cannot be dissolve in water.
A

1.

52
Q

interaction between molecules

A

Intermolecular force

53
Q

Hard and brittle, have high melting point and a poor thermal and electrical conductor like table salts.

A

Ionic crystalline

54
Q

Solids occupied by molecules whose forces between may be LDF, dipole-dipole or H-bond.

A

Molecular crystalline

55
Q

Glass is an example.

A

Amorphous solid

56
Q

The hardest of the substance belong to this type.

A

Network covalent

57
Q

Crystalline solid that is used as electric wires.

A

Metallic crystalline

Gen Chem (1 decks)

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