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Chemistry Tests > Chemistry Test chapter 9 cumulative > Flashcards

Chemistry Test chapter 9 cumulative Flashcards

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1
Q

Name the type of bond that results from sharing of four electrons.

A

Double bond

Covalent bond

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2
Q

Know the equation for ideal gas law.

A

PV=nRT

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3
Q

What is the heat required to cause a unit rise in the temperature of a unit mass of a given substance?

A

Specific heat

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4
Q

Absolute zero equals …

A

-273.15 degrees Celsius

0 kelvins

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5
Q

What causes the bright colored lines in the spectrum of glowing hydrogen gas?

A

Each line is a photon emitted when an electron drops to a lower energy level

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6
Q

What property is used to predict whether a bond is primarily ionic or primarily covalent?

A

Electronegativity

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7
Q

Name the principle that states elements tend to react chemically to achieve a noble gas electron configuration whether by losing, gaining, or sharing electrons.

A

Octet rule

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8
Q

Know and understand Exothermic chemical reactions.

A
  • chemical reaction releasing energy, usually causes the products to become hotter than the reactants because some energy was released.
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9
Q

Understand the differences between compounds and mixtures.

A

Compound- are combined in definite proportions , are chemically combined, lose their properties to form a new substance with new properties, can be separated only by chemical means

Mixtures- are present in variable proportions, are not chemically combined, each component retains its properties, can be separated by physical means

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10
Q

Name the covalent bond in which the bonding electron pair is pulled closer to the more electronegative element.

A

Polar bond

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11
Q

Understand the uncertainty principle.

A
  • it is impossible to simultaneously determine the momentum and the position of an electron with precision; either momentum or position may be measured precisely but not both.
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12
Q

Know and understand covalent bond.

A

Sharing of one or more electron pairs between two atoms

- atoms of non metals of similar Electronegativity

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13
Q

Know and understand ionic bond.

A

Electrostatic force of attraction between ions resulting from transfer of electrons
- atoms of metals and non metals having widely different electronegativites

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14
Q

Know and understand metallic bond.

A

Delocalized electron cloud around metal atoms

- atoms of metallic elements

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15
Q

True/false

The second law of thermodynamics states that enthalpy of the universe is always increasing.

A

False

Entropy (disorder)

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16
Q

True/false

The simplest repeating unit in a crystal is a unit cell.

A

True

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17
Q

True/false

The molecule of CO2 in which two polar bonds point symmetrically in opposite directions is polar.

A

False

Nonpolar

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18
Q

True/false

Kinetic energy is associated with an object’s position.

A

False

Potential energy

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19
Q

True/false

The speed of light in a vacuum is approximately 3.00 x 10 (8) m/s.

A

True

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20
Q

True/false

Atoms that are of the same element but differ in the number of particles in the nucleus are isotopes.

A

That differ in mass numbers

True

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21
Q

True/false

A solid whose particles are characterized by a regular, repeating, three dimensional pattern is an amorphous solid.

A

False

Crystalline solid

22
Q

Know formula for sodium sulfate.

A

Na2SO4

23
Q

Name the type of chemical formula that is the simplest ratio of atoms in a compound.

A

Empirical formula

Formula unit- called this when referring to ionic compounds

24
Q

What is PCI (5) - check test question number 30.

A

Phosphorous pentachloride

25
Q

What particle that composes an atom has a negative charge?

A

Electron

26
Q

Name the term that refers to a bonding situation in which electrons are shared by more that two atoms.

A

Delocalization

27
Q

How long is 2.54 cm in millimeters.

A

.254 milli meters

28
Q

Elements fluorine, brownie, and iodine are part of what category?

A

Halogens

29
Q

Elements like magnesium, calcium and barium are part of what category?

A

Alkaline Earth Metals

30
Q

What type of geometry does acetone in which three bonding pairs of electrons are arrayed around the central atom have?

A

Trigonal planar

31
Q

Which of the following elements would you expect to have the greatest electro negativity ? Is it S, Ca, CI and/or Cs.

A

Cl

32
Q

A +BC= AC+B

What kind of reaction?

A

Single displacement

33
Q

What type of geometry does hydrogen selenide which has two bonding pairs and two no binding pairs of electrons around the central atom have?

A

Angular

34
Q

Why does H2O have a higher boiling point than H2S?

A

Because oxygen has a higher Electronegativity causing its atoms to attract stronger than sulfur

35
Q

Elements boron, silicon and geranium are part of what category?

A

Semi metals

36
Q

Going from solid to liquid is what process?

A

Heat of fusion

Melting

37
Q

Know and understand dipole-dipole force.

A

Found only in polar molecules
Fairly strong
Constant attraction between weak partial charges

38
Q

Know and understand hydrogen bond.

A

Found only in molecules containing hydrogen covalently bonded to highly electronegative atoms
Very strong force
Constant attraction between relatively strong partial charges

39
Q

Know and understand London force.

A

Found in all molecules
Very weak force
Momentary attraction between weak partial charges

40
Q

The —— cubic arrangement of atoms in a crystal has the least empty space of any cubic arrangement.

A

Hexagonal close packing

41
Q

The ——– law of thermodynamics relates change in internal energy to heat and work.

A

First

42
Q

The outermost electrons in an atom which are involved in chemical bonding are called ——- electrons.

A

Valence

43
Q

The ——- theory of light states that light is electromagnetic waves traveling as bundles or packets of energy.

A

Quantum

44
Q

The mass of a substance per unit of volume is called ——.

A

Liters per mol

45
Q

A theoretical gas that exactly obeys the assumptions of the kinetic theory would be called a(n) ——— gas.

A

Ideal

46
Q

Know how to balance equations.

A

Good

47
Q

Know how to draw the Lewis structure of phosphorus trichloride.

A 
.  .         .  .      . .
            :Cl—     P  —Cl:
             . .          \        . .
                        :Cl:
                         . .
48
Q

Using the periodic table, calculate the molar mass of benzene.

A

C6H6

49
Q

See question 59.

A

Q

50
Q

A sample of helium gas has a volume of 620. mL at a temperature of 500. K. If we decrease the temperature to 100. K while keeping the pressure constant what will the new volume be?

A

P•V P•V
—- = —-
T T

51
Q

Hard substances like diamonds, silicon carbide and Quartz that contain covalent bonds but do not consist of discrete molecules are referred to as …

A

Crystalline solids- atoms or molecules regularly arranged

Chemistry Tests (10 decks)

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