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STUDY > GEN-CHEMISTRY > Flashcards

GEN-CHEMISTRY Flashcards

1
Q

Kinetic Molecular Theory

A

explains the properties of solids and liquids terms of intermolecular forces of attraction and the kinetic energy of the individual particles

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2
Q

Matter

A

made up of tiny particles and these particles are in constant motion. particles are proportional to temp. Increased temp means greater speed.

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3
Q

Intermolecular forces of attraction

A

attractive forces btwn molecules in solid and liquid states.

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4
Q

Types of Intermolecular forces

A

London Dispersion Forces
Dipole-Dipole Forces
Hydrogen Bond

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5
Q

London Dispersion Forces

A

weakest type. When 2 NON-POLAR molecules (approach) each other, dipole moment forms.

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6
Q

Dipole-Dipole Forces

A

exist in POLAR molecules. One end of dipole (attracts) the opposite charge end of other dipole

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7
Q

Hydrogen Bond

A

a strong type of dipole-dipole force that exists between hydrogen atoms. Hydrogen occurs in polar molecules. Containing H to NOF

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8
Q

SOLID

A

tightly packed arrangement of particles.

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9
Q

Types of Solid States

A

Arrangement of particles: Crystalline Solids and Amorphous Solids

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10
Q

Crystalline Solid State

A

Typical Geometry, 3-D, and has a definite arrangement of particles. (SODIUM CHLORIDE, QUARTS, DIAMOND, ETC.)

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11
Q

Properties of Crystalline Solids

A

Has a sharp melting point, definite shape, when cut- the new cut’ surfaces is smooth and plain, definite heat of fusion,

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12
Q

Types of Crystalline Solids

A

Molecular solids, metallic solids, ionic solids, and covalent solids.

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13
Q

Amorphous Solid State

A

the property of rigidity and incompressibility. Do not have a geometric form (glass, rubber, plastic) . Irregular surfaces and arrangement of particles

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14
Q

Solutions

A

Parts per Million, Mass or Volume Percent, Mole Fraction, Molarity, Molality

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15
Q

Parts Per Million

A

weight to weight ratio used to describe concentrations

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16
Q

Mass or Volume Percent

A

ratio of the mass of the solute present in a solution

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17
Q

Mole Fraction

A

unit of concentration. amount of solute and solvent are measured by the mole of fraction and presented as X

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18
Q

Molarity

A

the number of moles of dissolved solute per liter of solution. If divided by 1000 then molarity is expressed as the number of millimoles per milliliter of solution.

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19
Q

Molality

A

important properties of solutions. expresses the concentration of as solute in a solution and depends on the mass of the solvent. “Molal concentration”

20
Q

Chemical Kinetics

A

study of chemical processes and rates of reactions

21
Q

Chemical Reaction

A

process of reactants transforming into products. Written as chemical equation. Reactants on left and products on right.

22
Q

Concentration

A

amount of solute present in a given volume of solvent. More solute added, higher concentration. High concentration leads to faster chemical reactions because there are more particles available to react with each other.

23
Q

Difference between Solvent, Solute, and Solution

A

Solvent- substance
solute- the substance that gets dissolve in water
Solution- mixture of solvent + solute

24
Q

Collision Theory

A

reactants must collide with each other with sufficient energy and proper orientation

25
Q

Activation Energy (Ea)

A

minimum amount of energy required for a chemical reaction to occur

25
Q

Rate of Reaction

A

the speed at which the reactants formed into products in chemical reaction

26
Q

Factors of Reaction rate

A

catalysts, concentration, surface area, temperature

26
Q

Catalysts

A

speeds reaction without being used up and give another path for a faster chemical reaction

27
Q

Concentration

A

high concentration leads to faster chemical reaction

28
Q

Temperature

A

higher temperature speeds up reaction

29
Q

Surface area

A

more surface area, more contact for reactions

30
Q

Kinetic Energy

A

when an object is in motion, it possesses a kinetic energy and the amount of energy depends on its mass and speed.

31
Q

Covalent Bond

A

Sharing of electrons. When pair of electrons are shared by atoms

32
Q

Types of Catalyst

A

Homogeneous Catalysis (reactants are insame state of matter) and Heterogenenous Catalysis (not in same state of matter)

33
Q

Matter in the liquid phase

A

a state where they have definite volume but take the shape of their container

34
Q

What are the properties of matter in the liquid phase?

A

surface tension, viscosity, capillarity, vapor pressure, boiling point

35
Q

it allows to resist external force due to cohesive forces between molecule

A

surface tension

36
Q

the measure of a fluid’s resistance to deformation or flow

A

viscosity

37
Q

the ability of a liquid to flow in narrow spaces or tubes, contrary to the force of gravity

A

capillarity

38
Q

the pressure exerted by a vapor in equilibrium with its condensed phases (solid or liquid) in a closed system.

A

vapor pressure

39
Q

the temperature at which vapor pressure equals the external pressure, causing bubbles of vapor to form within the liquid

A

boiling point

40
Q

Give example of viscosity and explain how

A

A honey. Honey has high viscosity because it flows slowly.

41
Q

It forms a skin on water

A

Surface tension

42
Q

When a tube is dipped into the water, you’ll notice that the water inside it rises. What action does takes place?

A

Capillary action

43
Q

When a pot is heated on a stove, a water molecule gains enough energy to escape into the air (gas). What action does this takes place?

A

Vapor pressure

44
Q

When bubbles start to occur when a pot heated on a stove. It is called…

A

Boiling Point

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