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GEN CHEM > REVIEWER FOR 1ST QUARTER EXAM (GC2) > Flashcards

REVIEWER FOR 1ST QUARTER EXAM (GC2) Flashcards

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1
Q

explains the properties of liquids in term of the intermolecular forces of attraction and the kinetic energy of the individual particles

A

KINETIC MOLECULAR MODEL

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2
Q

refers to attractive forces between particles, it pull the particles together

A

INTERMOLECULAR FORCES

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3
Q

keep the particles at a distance and/or moving around

A

KINETIC ENERGY

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4
Q

PROPERTIES OF SOLID

A
  • Have definite shape and volume
  • Do not flow
  • Virtually incompressible
  • Expand when heated but to a lesser extent
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5
Q

PARTICLES OF SOLIDS

A
  • Strongly attached to each other
  • Vibrate in fixed positions
  • Vibrate faster when heated
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6
Q

PROPERTIES OF LIQUID

A
  • Have definite volume but no definite shape
  • Flow and take the shape of its container
  • Very difficult to compress
  • Slightly expand when heated
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7
Q

PARTICLES OF LIQUIDS

A
  • Weakly attached to each other; break their interaction easily
  • Move more freely that those in solids
  • Move faster when heated
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8
Q

Giving/taking electron, formula unit, force of attraction between two opposite charges (ions), keep the compound solid at room temperature

A

Ionic bond

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9
Q

sharing electrons, weaker only involves partial charges, molecules

A

Covalent Bond

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10
Q

Intermolecular Forces of Attraction in a pure substance include…

A
  • DIPOLE-DIPOLE FORCES
  • HYDROGEN BONDING
  • ION-DIPOLE
  • LONDON DISPERSION FORCES
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11
Q

Dipole-dipole and London dispersion forces are collectively known as

A

VAN DER WAALS FORCE

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12
Q

exists between two polar molecules or a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative

A

DIPOLE-DIPOLE FORCES

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13
Q

A special type of dipole-dipole interaction that exist only in molecules that contain H atom bonded to a small, highly electronegative atom such as N, O, or F

A

HYDROGEN BONDING

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14
Q

Acts between an ion (either positive or negative) and a polar molecule. The degree of this interaction depends on the a size and charge of the ion and on the size and dipole moment of the polar molecules; Cations (positively charged ions) interact more strongly with dipoles than anions (negatively charged ions)

A

ION-DIPOLE FORCES

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15
Q

The weakest IMF or simply dispersion forces are attraction that exist between all atoms and molecules

A

LONDON DISPERSION FORCES

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16
Q

The ease when they move within the atom is called?

A

Polarization

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17
Q

GENERAL PROPERTIES OF LIQUIDS

A
  • SURFACE TENSION
  • VISCOSITY
  • VAPOR PRESSURE
  • BOILING POINT
  • HEAT VAPORIZATION
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18
Q

It is the property of a liquid to resist an external force and thus assume a lesser surface area.
This attributed to the strong attractive and cohesive forces between and among the molecules, particularly at the surface of the liquid.

A

SURFACE TENSION

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19
Q

This is the resistance of a liquid to flow. It is loosely referred to as the thickness and thinness of a liquid.
The greater the intermolecular forces, the more viscous the substance
Example: Oil and honey

A

VISCOSITY

20
Q

the pressure exerted by its vapor when in equilibrium wit its liquid or solid. This means that when a solid substance is made to evaporate in a close container, the gas exerts a pressure above the liquid.
Substances with relatively strong IMF will have low vapor pressure because the particles will have difficulty escaping as a gas.

A

VAPOR PRESSURE

21
Q

temperature at which its vapor pressure is equal to the external atmospheric pressure. It is also influenced by the strength of its IMF. The greater the attractive forces, the higher the energy needed to increase the kinetic energy of the molecules to break these forces

A

BOILING POINT

22
Q

The temperature at which a liquid boils under an ______ of ________ is referred to as its normal boiling point

A

atmospheric pressure, of 760 mmHg (1 atm)

23
Q

The normal boiling point of water is ?

A

100 degree Celsius

24
Q

the amount of heat required to vaporize one mole of a substance at its boiling point.
The application of heat disrupts the intermolecular forces of attraction of the liquid molecules and allow them to vaporize.

A

MOLAR HEAT OF VAPORIZATION

25
Q

have a highly regular arrangement of particles

A

CRYSTALLINE SOLIDS

26
Q

a three dimensional system of points designating the positions of the components (atoms, ions or molecules) that make up a crystal.

A

LATTICE

27
Q

have considerable disorder in their structure. Such as glass, are formed rather rapidly that its constituent particles do not have time to align or organize into a more definite crystalline lattice

A

AMORPHOUS SOLIDS

28
Q

such as sodium chloride (NaCl), have ions at different points of lattice

A

IONIC SOLIDS

29
Q
  • such as sucrose (C₁₂H₂₂O₁₁) and ice (H₂O) has discrete covalently bonded molecule at each of its lattice points.
A

MOLECULAR SOLIDS

30
Q

such as gold, copper and bronze are composed of metal atoms bonded together by metallic bond

A

METALLIC SOLIDS

31
Q

are covalently bonded atoms that form a continuous network such as SiO2 and some of forms carbons such as graphite and diamond

A

COVALENT-NETWORK SOLIDS

32
Q

such as Krypton (Kr) and Argon (Ar) consists of atoms of noble gases held together by London dispersion forces

A

GROUP 8A SOLIDS

33
Q

6 PHASE CHANGES OF MATTER

A
  1. MELTING
  2. FREEZING
  3. EVAPORATION
  4. CONDENSATION
  5. SUBLIMATION
  6. DEPOSITION
34
Q

Point at which the temperature and
pressure allow for a substance to be a solid, liquid, and gas at the same time

A

TRIPLE POINT

35
Q

The highest point at which the
temperature and pressure can allow a substance to be both a liquid and a gas (any higher of a temperature/pressure and the substance cannot exist
as a liquid)

A

CRITICAL POINT

36
Q

a special fluid state of
substance, which refers to any substance at a
temperature and pressure above its critical point,
where distinct liquid and gas phases do not exist

A

SUPER CRITICAL FLUID

37
Q

SOLID PHASE OF CARBON DIOXIDE

A

DRY ICE

38
Q

CRITICAL POINT OF WATER

A

373.99

39
Q

CRITICAL PRESSURE OF WATER

A

217.75

40
Q

SOLID TO GAS

A

SUBLIMATION

41
Q

GAS TO SOLID

A

DEPOSITION

42
Q

GAS TO LIQUID

A

CONDENSATION

43
Q

LIQUID TO GAS

A

VAPORIZATION/EVAPORATION

44
Q

LIQUID TO SOLID

A

FREEZING

45
Q

SOLID TO LIQUID

A

MELTING

GEN CHEM (2 decks)

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