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CHEM111 > MIDTERM (chp5-7) > Flashcards

MIDTERM (chp5-7) Flashcards

1
Q

Ions

A

Formed when electrons are added to, or removed from a neutral species

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2
Q

Cation

A

A positively charged ion resulting from removing 1 or more electrons from a neutral species

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3
Q

Anion

A

A negatively charged ion resulting from a neutral specie gaining one or more electron

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4
Q

Octet rule

A

In forming compounds, atoms of elements lose, gain, or share electrons in such a way as to produce a noble gas electron configuration for each of the atoms involved

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5
Q

Group 1A Alkali Metals:

A
  • All the alkali metal elements tend to lose 1 electron to form a +1 cation
  • Cation has the same electron configuration as the preceding noble gas element
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6
Q

Group 2A Alkaline Earth Metals:

A

All alkaline earth metal elements tend to lose 2 electrons to form 2+ cations with the same electron configuration as the preceding noble gas element

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7
Q

Group 17 Halogens:

A
  • All halogen elements tend to gain 1 electron to form 1 anion with the same electron configuration as the next noble gas element
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8
Q

Binary Ionic compounds

A

Contains two monoatomic ions

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9
Q

Smaller number of oxygen prefix

A

ite (eg. sulfITE)

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10
Q

Larger number of oxygen prefix

A

Ate (eg. sulfATE)

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11
Q

Number suffix

A
  • mono 1
  • di 2
  • tri 3
  • tetra 4
  • penta 5
  • hexa 6
  • hepta 7
  • octa 8
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12
Q

Bonding electrons

A

Valence electrons that are shared between two nuclei in a covalent bond

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13
Q

Nonbonding electrons

A

Valence electrons that are not involved in a bond (ione pairs)

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14
Q

Single covalent bond

A

Two atoms that share 1 pair of valence electrons

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15
Q

Single covalent bond

A

Two atoms that share 1 pair of valence electrons

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16
Q

Double covalent bond

A

Two atoms that share 2 pairs of valence electrons

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17
Q

Triple covalent bond

A

Two atoms that share 3 pairs of electrons

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18
Q

Coordinate covalent bond

A

a covalent bond (a shared pair of electrons) in which both electrons come from the same atom.

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19
Q

Non oxyacids

A

Contain hydrogen and one or more non metals, but not oxygen

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20
Q

Oxyanions

A

Polyatomic ions containing oxygen. When writing, add suffix ATE

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21
Q

Ionic bond

A

Force of attraction between oppositely charged ions

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22
Q

Ionic compound

A

Compound composed of oppositely charged ions

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23
Q

Ionic lattice

A

Ionic compounds that contain many cations and anions packed together in a structure of alternating positive and negative charges that stretch out in three dimensions

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24
Q

Chemical formula

A

Tells us how many atoms of each element are in a compound

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25
Q

Empirical formula

A

Tells us the smallest number of ions necessary to form a compound

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26
Q

Covalent bond

A

When two nonmetal atoms come together

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27
Q

The Magnificent Seven (Elements that form Diatomic Molecules)

A
  • Hydrogen H2
  • Nitrogen N2
  • Oxygen O2
  • Fluorine F2
  • Chlorine Cl2
  • Bromine Br2
  • Iodine I2
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28
Q

Solution

A

Result of when a substance such as salt or sugar mixes with water and disperses through the liquid to form a homogeneous mixture

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29
Q

Aqueous solution

A

If the liquid is water

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30
Q

Soluble

A

Compounds that dissolve in water

31
Q

Insoluble

A

Compounds that do not dissolve in water

32
Q

Electrolyte solutions

A

Another name for aqueous ionic solutions because if ionic compounds are dissolved in water, the resulting solutions conduct electricity much more efficiently

33
Q

Dissociation

A

When ionic compounds dissolve in water and the positive/negative ions are pulled away from each other and surrounded by water ions

34
Q

Acids

A

Covalent compounds that produce H+ ions in aqueous solution

35
Q

Base

A

Covalent compounds that produce OH- ions in aqueous solution

36
Q

Reactants

A

Substances as they exist before the chemical reaction (starting materials)

37
Q

Products

A

Substances present after the chemical reaction

38
Q

Important symbols:

A
  • (S): solid
  • (g): gas
  • (l): liquid
  • (aq): aqueous solution (dissolved in water)
39
Q

Synthesis reaction

A

When two reactants join together to form a single product

40
Q

Decomposition reaction

A

When a single reactant forms two or more products

41
Q

Single replacement reaction

A

When one element replaces another element in a compound

42
Q

Double replacement reaction

A

When two compounds rearrange to form two new compounds (swap of cation-anion pairs)

43
Q

Combustion reaction

A

a reaction in which a substance reacts with oxygen gas, releasing energy in the form of light and heat.

44
Q

Acid base neutralization reactions

A

Acid + base –> salt + water

45
Q

Oxidation reduction reactions

A

Reactions involving a transfer of electrons

46
Q

Electrolyte

A

Substance whose aqueous solutions conduct electricity due to presence of charged particles (ions) in solution (eg. Aqueous solutions of ionic compounds)

47
Q

Non electrolyte

A

Substance whose aqueous solution does not conduct electricity (eg. Aqueous solutions of molecular compounds)

48
Q

Precipitation Reactions

A

When two aqueous solutions combine to produce a solid (insoluble) product

49
Q

Saturated solution

A

Solution that contains the maximum amount of dissolved solute and any more solute added will remain undissolved

50
Q

Unsaturated solution

A

solution that contains less than the maximum amount of solute that is capable of being dissolved.

51
Q

When an atom is oxidized, it…..

A

Loses electrons

52
Q

When an atom is reduced, it…..

A

Gains electrons

53
Q

Hydrocarbons

A

compounds comprised exclusively of carbon and hydroge

54
Q

Complete ionic equation

A

Equation showing all ions present in a solution

55
Q

Spectator ions

A

An ion that is present in a solution but not directly involved in a chemical change

56
Q

Net ionic

A

an equation that depicts only the molecules or ions that are actively involved in the reaction or those that undergo a change. In this equation, the spectator ions are not present

57
Q

Neutralization reactions

A

A reaction in which an acid and base combine; acids and hydroxide bases combine to produce water and an ionic compound

58
Q

Formula mass

A

Sum of atomic masses of atoms in one formula unit. Atomic masses are obtained from the periodic table in amu (atomic mass units)

59
Q

Percent composition from formula (3)

A
  • The percentage (by mass) of each element in a compound
  • Divide mass of one element in a compound by the total mass of a compound and then convert to percent
  • Mass of one element/mass of entire compound x 100%
60
Q

Molar mass of an element

A

the atomic mass in g/moL

61
Q

Chemical stoichiometry

A

Uses the amount of one substance to predict the amount of another substance that is consumed or produced, according to the balanced equation

62
Q

Theoretical yield

A

Amount of product that can form in a chemical reaction based on the balanced equation and the amount of starting materials present

63
Q

Actual yield

A

Amount of product that a chemist actually isolates from an experiment

64
Q

Percent yield

A

Gives information on how well the reaction is working

65
Q

Percent yield calculation

A

Actual yield/theoretical yield x 100%

66
Q

Mass spectrometry

A

Technique used to measure the mass of a molecule

67
Q

3 components of a mass spectrometry

A
  • Ionizing chamber
  • Electric field
  • Detector
68
Q

Elemental analysis

A

A technique used to determine the percent composition of a substance. It uses combustion reactions to convert compounds into simpler products (carbon dioxide, water, etc). The mass of each product indicates the percentage of each element in a sample

69
Q

Mole

A

A quantity consisting of 6.02 x 10^23 units

70
Q

Avogadro’s number

A

Number of particles in a mole; 6.02 x 10^23

71
Q

Molar mass

A

When a mass is expressed in grams per mole

72
Q

Excess reagent

A

Reagent that is present in largest stoichiometric quantities than the other reagents. So the substance that is not completely consumed

73
Q

Limiting reagent

A

Reagent that is completely consumed and limits the amount of product that can form

CHEM111 (6 decks)

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