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Gen Chem 2 > Lesson 1-4 > Flashcards

Lesson 1-4 Flashcards

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1
Q

At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is a solid. This is because

A

Dispersion interactions increase with molecular size.

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2
Q

Which one of the following molecules would be most polar?

A

HF

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3
Q

Which of the following forces that hold the atoms together in a molecule?

A

Intramolecular Forces

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4
Q

Which of the following IMFs occur between hydrogen and nitrogen?

A

Hydrogen Bond

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5
Q

are the attractive forces that act between molecules or particles.

A

Intermolecular Forces

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6
Q

Who is the proponent of the London Dispersion Force?

A

Fritz London

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7
Q

The kind of attraction that explains the dissolving of sodium chloride in water is

A

Ion-dipole

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8
Q

The forces of attraction that exist between nonpolar molecules are called

A

London dispersion force

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9
Q

is a theory that helps to explain observable properties and behaviors of solids, liquids,
and gases.

A

Kinetic Molecular Theory

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10
Q

1.

A type of intermolecular attraction—attractions between two polar molecules is called

A

Dipole-dipole force

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11
Q

The boiling point of water is about 200°C higher than one would predict from the boiling points of
hydrogen sulfide and hydrogen selenide. One may explain this apparent anomaly by which of the
following?

A

The intermolecular attractive forces are much greater in water than in hydrogen sulfide and
hydrogen selenide.

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12
Q

Why is the normal boiling point of hydrogen fluoride so much higher than that of hydrogen chloride,
the hydride of the next element in group VIIA?

A

The HF molecules undergo a higher degree of hydrogen bonding than HCl.

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13
Q

A friend in your chemistry class is struggling to understand why crystalline solids are grouped into
four main types: network, molecular, ionic, and metallic. Which explanation below will BEST help
him/her begin to understand why chemists might have these groups?

A

Crystalline solids all share a lattice structure, but the bonds that hold them together at the
atomic level differ. The elements that make up the solids also differ. These differences affect how a
solid conducts heat and electricity, and its density.

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14
Q

An engineer is designing an electrical system and is looking for a material to transmit energy. She
has four solids available, each made with different materials. To conduct energy most efficiently and
effectively, what material she should use?

A

Materials whose electrons are held with metallic bonds.

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14
Q

Which of the following is not a property of gases?

A

Gases are weightless near the surface of the earth

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15
Q

Which of the following has dispersion forces as its only intermolecular force?

A

CH4

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16
Q

The characteristics of gases needed to describe a gas completely include all the following

A

Pressure, Temperature, Volume

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17
Q

An engineer is designing an electrical system and is looking for a material to transmit energy. She
has four solids available, each made with different materials. To conduct energy most efficiently and
effectively, what material she should use?

A

Materials whose electrons are held with metallic bonds

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18
Q

A statement that is true about solids

A

All solids maintain a defined shape and size if conditions remain constant.

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19
Q

If the amount and temperature of a gas are kept constant, what do you think will happen to the
pressure and volume of the gas?

A

The pressure and volume of gas will be inversely proportional.

20
Q

The concept of “like dissolves like” is illustrated by

A

Polar solute will be soluble in a polar solvent

21
Q

A phase transitions should release the most energy is

A

Gas to solid

22
Q

What happens to particles when they are heated?

A

They speed up and spread-out

23
Q

particles travel in a straight line unless they collide with other particles or the walls of the
container

A

Gas

24
Q

is a special type of dipole–dipole force that exists between a hydrogen atom bound to a
small highly electronegative non-metal atom.

A

Hydrogen Bond

25
Q

is the intermolecular attraction between like or the same molecules.

A

Cohesion

26
Q

When a solution is completely dissolved and forms ions it is called a _______ solution.

A

electrolyte

27
Q

solids are arranged in fixed geometric patterns or lattices.

A

crystalline

28
Q

It is a measure of the elastic force in the surface of a liquid.
It is the amount of energy required to stretch or increase the surface of a liquid by a unit area.

Intermolecular forces of matter and properties of liquids

A

Surface tension

29
Q

is the tendency of a liquid to rise in narrow tubes or be drawn into small openings such as those between grains of a rock.

Intermolecular forces of matter and properties of liquids

A

Capillary action

30
Q

it is the pressure exerted by its vapor when in equilibrium with liquid or solid.

Intermolecular forces of matter and properties of liquids

A

Vapor pressure

31
Q

Defined as the resistance of a liquid to flow.
It is loosely referred to as the thickness and thinness of a liquid.

Intermolecular forces of matter and properties of liquids

A

Viscosity

32
Q

is the temperature at which a solid changes into a liquid.

Properties of Solid

A

Melting Point

33
Q

are non-crystalline solid in which the atoms and molecules are not organized in a definite lattice pattern.

Types of Solids

A

Amorphous Solid

34
Q

can be defined as the pressure at which the rate of sublimation of a solid matches the rate of deposition of its vapor phase.

Properties of Solid

A

Vapor Pressure of a Solid

35
Q

are arranged in a regular repeating pattern.

Types of Solids

A

Crystalline Solid

36
Q

consist of metal cations surrounded by a “sea” of mobile valence electrons.

Types of Crystalline Solids

A

Metallic Crystals

37
Q

consists of alternating positively-charged cations and negatively-charged anions

Types of Crystalline Solids

A

Ionic Crystals

38
Q

consist of molecules at the lattice points of the crystal, held together by relatively weak intermolecular forces

Types of Crystalline Solids

A

Molecular Crystals

39
Q

consists of atoms at the lattice points of the crystal, with each atom being covalently bonded to its nearest neighbor atoms.

Types of Crystalline Solids

A

Covalent Network Crystals

40
Q

is the property shown by substances which have molecules or ions that can assume more than one stable arrangement in the solid state.

A

Polymorphism

41
Q

is the change of the physical state of matter from the gas phase into the liquid phase, and is the reverse of vaporization.

A

Condensation

42
Q

is the transition of a substance directly from the solid to the gas state, without passing through the liquid state.

A

Sublimation

43
Q

is the phase transition in which gas transforms into solid without passing through the liquid phase.

A

Deposition

44
Q

Three types of Solubility

A
  1. Soluble
  2. Sparingly soluble
  3. Insoluble
45
Q

is a mixture of two or more substances, but it’s not just any mixture. A solution is a homogeneous mixture. In a homogeneous mixture, the dissolved particles are spread evenly through the mixture.

A

Solutions

46
Q

are ionic compounds that dissolves to form ions in solution completely.

Classification of Solutions

A

Electrolytes

47
Q

are the solutions that contain neutral molecules and do not dissociate into ions in solution.

Classification of Solutions

A

Nonelectrolytes

48
Q

Energy of Solution Formation

A
  1. Solute-solute interaction
  2. Solvent-solvent interaction
  3. Solute-solvent interaction

Gen Chem 2 (1 decks)

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