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1011 chem Flashcards

1
Q

Alkane

A

CnH2n+2

consist entirely of single-bonded carbon and hydrogen atoms and lack any other functional groups

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2
Q

Alkene

A

contains at least one carbon to carbon double bond (one o bond and one pi bond) (CnH2n)

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3
Q

Hydrocarbon nomenclature rules

A
  • identify longest chain
  • add prefix to indicate location of substituent
  • number carbon atoms in the chain by counting form end nearest to the substituents
  • substituents are listed alphabetically
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4
Q

isomer

A

Any 2 molecules with the same molecular formula but with different molecular
arrangement

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5
Q

functional Groups

A

An atom or cluster of atoms that are covalently bonded to carbon
- Affects the chemical behavior or specific properties of organic compounds
(e.g. polarity, acidity

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6
Q

Chiral Carbons

A

tetrahedral carbons linked to 4 different functional groups

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7
Q

amine

A

functional group where a Nitrogen atom is attached to a carbon/ Hydrogen atom

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8
Q

amide

A

Functional group where a Nitrogen atom is connected to a carbonyl carbon (C=O)

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9
Q

What is Thermodynamics

A

The branch of physical science that deals with the relations between
heat and other forms of energy (such as mechanical, electrical, or
chemical energy), and, by extension, of the relationships between all
forms of energy.

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10
Q

Isolated system

A

exchanges neither matter nor energy with its surroundings

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11
Q

Closed System

A

exchanges energy but not matter with its surroundings

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11
Q

Open system

A

exchanges both energy and matter with its surroundings

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11
Q

Chemical Change

A

always produces at least one type of matter that was not present before the change

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11
Q

Physical Change

A

a change in the state or properties of matter without
any accompanying change in its chemical composition

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12
Q

Types of energy

A

MELTS- NC

Mechanical
Electrical
Light/ Radiation
Thermal/ Heat
Sound
Nuclear
Chemical

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13
Q

Zeroth law of thermodynamics

A

– If two thermodynamic systems are each in thermal equilibrium
with a third, then they are in thermal equilibrium with each other
– If a = b and b = c, then a = c

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14
Q

First Law of thermodynamics

A

– Energy is conserved; it can neither be created nor destroyed,
just changed from one form to another

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15
Q

Second Law of thermodynamics

A

In all natural processes, the entropy of the universe increases
** Entropy means randomness/ lack of predictability

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16
Q

Third law of thermodynamics

A

– The temperature of a system cannot reach absolute zero
(−273.15°C, 0 K)

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17
Q

Exothermic chemical reaction

A

Reactions that release heat with a product of heat.
- Increased heat causes shift to the left and and vice versa

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18
Q

Endothermic Chemical Reaction

A

Reactions consume energy, heat is a reactant.
- increased heat causes shift to the right and vice versa

19
Q

Calorie

A

Amount of heat required to raise the temperature of 1 gram of water by 1 degree (1K)

1 calorie = 4.184 joules
1 kilocalorie (Calorie) = 4.184 kilojoules (kJ)

20
Q

Joule (SI unit)

A

The amount of energy used when a force of 1 newton (the force needed to
accelerate one kilogram of mass at the rate of one metre per second-squared
in the direction of the applied force) moves an object 1 m

21
Q

Enthalpy (H)

A

the sum of a system’s internal energy (U = heat + work) and the
product of its pressure (P) and volume (V) (expansion-compression work):
H = U + PV
We cannot measure enthalpy directly, but we can measure the changes

22
Chemical Equilibrium
when the rate of the forward reaction equals the rate of the reverse reaction
23
Reaction Quotient (Qc)
The amount of products relative to the amount of reactants at a particular point in the reaction (square brackets means concentration)
24
Equilibrium constant (Kc)
Tells us whether a reaction has a higher concentration of reactants or products as equilibrium.  Kc >> 1 at equilibrium the mixture contains mostly products  Kc << 1 at equilibrium the mixture contains mostly reactants
25
Acid- base reaction
hydrogen ion, H+ is transferred from one chemical species to another.
26
strong vs weak acids
strong= disassociate completely into it's constituent ions in aqueous solutions weak= does not disassociate completely
27
Strong VS Weak Base
Strong= accepts all donated protons, completely ionises in aqueous solution Weak= only some molecules accept protons
28
Acid- Ionisation constant (Ka)
the greater the Ka of an acid, the larger the concentration of H3O+, and therefore acid strength
29
Base-ionisation constant (Kb)
The larger the Kb of an base, the larger the concentration of OH- and the strength of the base
30
neutralisation reaction
type of acid-base reaction in which the reactants are an acid and a base, the products are often a salt and water, and neither reactant is the water itself
31
Binary Acids (Hydrogen+ Non- Metal compound)
– The word “hydrogen” is changed to the prefix hydro- – The other nonmetallic element name is modified by adding the suffix -ic – The word “acid” is added as a second word
32
Oxyacids (H+O+ at least 1 non- metal)
– Omit “hydrogen” – Start with the root name of the anion – Replace –ite with –ous – Replace –ate with –ic, – Add “acid
33
Buffer solution
Readily absorb excess H+ or OH-, keeping the pH of the body carefully maintained in the narrow range required for survival. - Mix of weak acid+ it's conjugate base - Weak base+ it's conjugate acid
34
pKa (Disassociation constant)
tells us the range where a buffer solution is useful - The pKa of a buffer is the pH when the concentrations of the two buffering species are equal, and where the maximum buffering capacity is achieved.
35
Properties of liquids
- cohesive forces - surface tension - adhesive forces - capillary action
36
Phase transition
Physical change from one state to another  Vaporisation and condensation  Boiling points  Melting and freezing  Sublimation and deposition
37
Factors that influence reaction rates (STIICCP)
-SA of the substances -Temperature -Instantaneous rate -Initial rate -Chemical nature/ reactivity -Concentration of reactants/ products -Presence of a catalyst
38
Precipitation
Dissolved substances react to form one (or more) solid products
39
Acid-base
Hydrogen ions, H+, are transferred from one chemical species to another
40
Oxidation-reduction (REDOX)
- Reactions where one or more elements involved undergo a change in oxidation number (involves transfer of electrons) - Oxidation = loss of electrons; Reduction = gain of electrons
41
Oxidation Number
- ON of an elemental substance= 0 - ON of a monatomic ion= same as ions charge - Sum of ONs= charge of the molecule/ ion Oxidation = increase in ON Reduction = decrease in ON
42
Solubility
Max amount of solute that may be dissolved in a solvent at a certain temperature. - When no more solute can be dissolved= saturated solution
43
Molarity (M)
No. of moles of solute in exactly 1 liter (1 L) of the solution M (mol/L) = n / V (L) moles = M (mol/L) x V (L) m (g) = n x Mr
44
Chemical changes types (DACC)
- Decomposition - Acid- Base - Combustion - Combination (synthesis)
45
Ionic Bond
an atom gives up electrons to another atom, electric charge attracts them -metal + non-metal
46
Covalent
Atoms share electrons - metal + metal
47
Electronegativity
The difference in electronegativity values (ΔEN) is used to determine whether the bond and molecule are polar (ΔEN 0.4 – 1.8) or non-polar (ΔEN < 0.4)
48
What the the 10 prefixes?
1 = mono- (sometimes omitted) 2 = di- 3 = tri- 4 = tetra- 5 = penta- 6 = hexa- 7 = hepta- 8 = octa- 9 = nona- 10 = deca
49
BOHR model
- This model worked for hydrogen atoms (single proton, single electron) - Bohr’s equation for predicting the structure of an atom did not apply to the next simplest atom, He that has two protons and two electrons

1011 (2 decks)

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