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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
Empirical formula
Tells us the smallest number of ions necessary to form a compound
26
Covalent bond
When two nonmetal atoms come together
27
The Magnificent Seven (Elements that form Diatomic Molecules)
- Hydrogen H2 - Nitrogen N2 - Oxygen O2 - Fluorine F2 - Chlorine Cl2 - Bromine Br2 - Iodine I2
28
Solution
Result of when a substance such as salt or sugar mixes with water and disperses through the liquid to form a homogeneous mixture
29
Aqueous solution
If the liquid is water
30
Soluble
Compounds that dissolve in water
31
Insoluble
Compounds that do not dissolve in water
32
Electrolyte solutions
Another name for aqueous ionic solutions because if ionic compounds are dissolved in water, the resulting solutions conduct electricity much more efficiently
33
Dissociation
When ionic compounds dissolve in water and the positive/negative ions are pulled away from each other and surrounded by water ions
34
Acids
Covalent compounds that produce H+ ions in aqueous solution
35
Base
Covalent compounds that produce OH- ions in aqueous solution
36
Reactants
Substances as they exist before the chemical reaction (starting materials)
37
Products
Substances present after the chemical reaction
38
Important symbols:
- (S): solid - (g): gas - (l): liquid - (aq): aqueous solution (dissolved in water)
39
Synthesis reaction
When two reactants join together to form a single product
40
Decomposition reaction
When a single reactant forms two or more products
41
Single replacement reaction
When one element replaces another element in a compound
42
Double replacement reaction
When two compounds rearrange to form two new compounds (swap of cation-anion pairs)
43
Combustion reaction
a reaction in which a substance reacts with oxygen gas, releasing energy in the form of light and heat.
44
Acid base neutralization reactions
Acid + base --> salt + water
45
Oxidation reduction reactions
Reactions involving a transfer of electrons
46
Electrolyte
Substance whose aqueous solutions conduct electricity due to presence of charged particles (ions) in solution (eg. Aqueous solutions of ionic compounds)
47
Non electrolyte
Substance whose aqueous solution does not conduct electricity (eg. Aqueous solutions of molecular compounds)
48
Precipitation Reactions
When two aqueous solutions combine to produce a solid (insoluble) product
49
Saturated solution
Solution that contains the maximum amount of dissolved solute and any more solute added will remain undissolved
50
Unsaturated solution
solution that contains less than the maximum amount of solute that is capable of being dissolved.
51
When an atom is oxidized, it.....
Loses electrons
52
When an atom is reduced, it.....
Gains electrons
53
Hydrocarbons
compounds comprised exclusively of carbon and hydroge
54
Complete ionic equation
Equation showing all ions present in a solution
55
Spectator ions
An ion that is present in a solution but not directly involved in a chemical change
56
Net ionic
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
Neutralization reactions
A reaction in which an acid and base combine; acids and hydroxide bases combine to produce water and an ionic compound
58
Formula mass
Sum of atomic masses of atoms in one formula unit. Atomic masses are obtained from the periodic table in amu (atomic mass units)
59
Percent composition from formula (3)
- 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
Molar mass of an element
the atomic mass in g/moL
61
Chemical stoichiometry
Uses the amount of one substance to predict the amount of another substance that is consumed or produced, according to the balanced equation
62
Theoretical yield
Amount of product that can form in a chemical reaction based on the balanced equation and the amount of starting materials present
63
Actual yield
Amount of product that a chemist actually isolates from an experiment
64
Percent yield
Gives information on how well the reaction is working
65
Percent yield calculation
Actual yield/theoretical yield x 100%
66
Mass spectrometry
Technique used to measure the mass of a molecule
67
3 components of a mass spectrometry
- Ionizing chamber - Electric field - Detector
68
Elemental analysis
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
Mole
A quantity consisting of 6.02 x 10^23 units
70
Avogadro's number
Number of particles in a mole; 6.02 x 10^23
71
Molar mass
When a mass is expressed in grams per mole
72
Excess reagent
Reagent that is present in largest stoichiometric quantities than the other reagents. So the substance that is not completely consumed
73
Limiting reagent
Reagent that is completely consumed and limits the amount of product that can form

CHEM111 (6 decks)

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