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Chemistry Flashcards

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1
Q

where is all energy originated from?

A

the sun

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2
Q

what is an exothermic reaction?

A

A change in a chemical energy where energy/heat EXITS the
chemical system
Results in a decrease in chemical potential energy
Reactants Ep > Products Ep
Molar enthalpy < 0
Enthalpy change < 0
energy in products

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3
Q

what is an endothermic reaction?

A

A change in chemical energy where energy/heat ENTERS the chemical system
Results in an increase in chemical potential energy
Reactants Ep < Products Ep
Molar enthalpy > 0
Enthalpy change > 0
energy in reactants

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4
Q

what is kinetic energy, potential energy, thermal energy, temperature, and heat?

A

kinetic: energy of molecular motion
potential: energy stored in bonds and inter molecular forces
thermal: total kinetic energy of all particles in a system, increases with temp
temperature: average kinetic energy of particles in a system
heat: transfer of thermal energy. Heat is not possessed by
a system. Heat is energy flowing between systems.

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5
Q

how to calculate change in thermal energy? what does a negative value or positive value indicate?

A

Q = mcAT
negative Q value -> exothermic, heat lost by system, temp of system decreases, temp of surrounding increases
positive Q value -> endothermic, heat gained by system, tmep of system increases, temp of surrounding

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6
Q

how to calculate enthalpy change?

A 
ArH = mcAT
ArH = nArHm
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7
Q

how to calculate molar enthalpy using calorimetry?

A

nAcHm = mcAt (right side is chemical system, left side is surroundings)
n -> moles of fuel
AcHm -> molar enthalpy of combustion of fuel
m -> mass of water
c -> specific heat capacity of water
At -> temprature of water

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8
Q

what are the 4 ways of communicating enthalpy?

A
  1. state molar enthalpy of a specific reactant
  2. balanced chemical reaction with enthalpy change written next to it
  3. including the enthalpy change in the balanced chemical reaction
  4. potential energy graph
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9
Q

how to do Hess’ Law?

A

to determine the enthalpy change of a reaction, you can use the the given enthalpies of similar reaction.
you can manipulate the given reactions to ‘form’ the unknown enthalpy reactions

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10
Q

how to find the molar enthalpy using molar enthalpy of formations?

A

ArH = ((moles of product C)(molar enthalpy of formation of product C)) + ((moles of product D)(molar enthalpy of formations of product D)) - ((moles of reactant A)(molar enthalpy of formation of reactant A)) + ((moles of reactant B)(molar enthalpy of formations of reactant B))

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11
Q

what is activation energy? how to interpret a graph?

A

The minimum collision energy required for effective collision
on graph it is the distance from the reactant to the activated complex
exothermic –> reactants < products, Ea > ArH
endothermic –> reactants < products, Ea < ArH

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12
Q

what are catalysts and how does it affect reaction rate?

A

A catalyst is a substance that increases the rate of a chemical reaction without being consumed itself in the overall process

A catalyst reduces the quantity of energy required to start the reaction, and results in a catalyzed reaction producing a greater yield in the same period of time than an uncatalyzed reaction.
It does not alter the net enthalpy change for a chemical reaction

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13
Q

what is a redox reaction?

A

Is a chemical reaction in which electrons are transferred

Must have both reduction and oxidation happening for the reaction to occur

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14
Q

what is reduction and oxidation? what are the reducing and oxidixing agents?

A

reduction –> gain of electrons
oxidation –> loss of electrons
reducing agent –> causes reduction by losing electrons (is oxidized)
oxidizing agent –> causes oxidation by gaining electrons (is reduced)

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15
Q

how to build a redox table?

A

use the spontaneity rule.
if the the reaction occurs and is spont. the OA will be above the RA
if the reaction does not occur and is non spont. the OA will be below the RA

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16
Q

how to predict redox reactions?

A

use the five step method.

  1. list ALL entities
  2. identify all possible OA’s and RA’s
  3. find the SOA and SRA
  4. write there half reactions
  5. balance and add them and predict spontaneity
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17
Q

how to redox stoichiometry?

A
  1. list entities present
  2. find SOA and SRA
  3. write half reactions, balance electrons, add them
  4. use the given ration and multiply by ratios to find the missing
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18
Q

how to predict reaction for acidic solutions?

A
  1. balance everything but the hydrogens and oxygens
  2. use H2O to balance oxygens and H+ to balance hydrogens
  3. balance charge by adding electrons
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19
Q

what are oxidation states?

A

The oxidation number of a free element is always 0.
The oxidation number of a monatomic ion equals the charge of the ion.
Fluorine in compounds is always assigned an oxidation number of -1.
Oxygen almost always has an oxidation number of -2, except in peroxides (H2O2) where it is -1 and in compounds with fluorine (OF2) where it is +2.
Hydrogen has an oxidation number of +1 when combined with non-metals, but it has an oxidation number of -1 when combined with metals.
The algebraic sum of the oxidation numbers of elements in a compound is zero.
The algebraic sum of the oxidation states in an ion is equal to the charge on the ion

20
Q

what are disproportionate reactions?

A

a single substance that is both oxidized and reduced
has to GAIN and LOSE electrons
oxidation number will go up and down

21
Q

what are 6 properties of a voltaic cell? what does it look like?

A
  • spontaneious
  • positive Ecell
  • at cathode (positive electrode) SOA undergoes reduction
  • at anode (negative electrode) SRA undergoes oxidation
  • electron move from anode –> cathode
  • anions –> anode, cations –> cathode
    consists of two‐half cells separated by a porous boundary with solid electrodes connected by an external circuit
22
Q

what is a standard cell and how to solve for cell potentials?

A

A standard cell is a voltaic cell where each ½ cell contains all entities necessary at SATP conditions and all aqueous solutions have a concentration of 1.0mol/L
Standard Cell Potential, Ecell= the electric potential difference of the cell (voltage)
Ecell=Er cathode–Er anode
• Where Er is the standard reduction potential, and is a measure of a standard ½ cell’s ability to attract electrons.
• The higher the Er, the stronger the OA
• All standard reduction potentials are based on the standard hydrogen ½ cell being 0.00V.
This means that all standard reduction potentials that are positive are stronger OA’s than
hydrogen ions and all standard reduction potentials that are negative are weaker.
• If the Ecell is positive, the reaction occurring is spontaneous.
• If the Ecell is negative, the reaction occurring is non‐spontaneous

23
Q

what are 6 properties of electrolyic cell?

A
  • non spont
  • negative Ecell
  • at cathode (negative electrode) SOA undegoes reduction
  • at anode (positive electrode) SRA undergoes oxidation
  • electrons move from anode –> cathode
  • anions –> anode, cations –> cathode
24
Q

what is the chloride anomaly?

A

occurs during electrolysis of solutions containing the chloride ion
since water is the SRA water, it should react at the anode and get oxidized however chloride ions do this instead
chlorine gas is produced instead of oxygen gas in situations where chloride and water are the only reducing agents present

25
Q

how to do half cell calculations?

A
  1. write out the balanced half reaction
  2. use the molar ratio to convert the chemical amount of one substance to another
  3. convert to the missing quantity
    ne = Vt/F
    v = amps
    t = time (s)
    F = 9.65 x 10^4
26
Q

how to balance reactions using oxidation states?

A

Step 1. Write down the unbalanced equation
Step 2. Separate the redox reaction into half-reactions
a) Assign oxidation numbers for each atom
b) Identify and write out all redox couples in reaction
c) Combine these redox couples into two half-reactions
Step 3. Balance the atoms in each half reaction
a) Balance all other atoms except H and O
b) Balance the oxygen atoms with H2O
c) Balance the hydrogen atoms with H+
d) In a basic medium, add one OH- to each side for every H+
Step 4. Balance the charge with e-
Step 5: Make electron gain equivalent to electron loss in the half-reactions
Step 6: Add the half-reactions together
Step 7: Simplify the equation

27
Q

what compounds are not organic?

A

carbonate ions CO3-
carbides (carbon bonded to metal)
oxides of carbon
cyanide (CN)

28
Q

what are the 4 types of formulas?

A
  1. molecular formula
  2. structural formula (every bond)
  3. condensed structural formula (bonds for carbons only)
  4. line diagrams
29
Q

what are alkanes, alkenes, alkynes?

A

alkanes -> only single carbon bonds, CnH2n+2, saturated
alkenes -> double carbon bonds present, CnH2n, unsaturated
alkynes -> triple carbon bonds present, CnH2n-2, unsaturated

30
Q

how to name alkanes?

A
  1. Find the parent chain. Use the appropriate root and suffix.
  2. Number the parent chain carbon atoms, starting from the end closest to the branch(es) so that the numbers are the lowest possible
  3. Identify any branches and their location number on the parent chain (use the suffix–yl for branches)
  4. If more than one of the same branch exist, use a multiplier(di,tri) to show this.Remember to include all numbers
  5. If different branches exist, name them in alphabetical order
  6. Separate numbers from numbers using commas, and
    numbers from words using dashes (no extra spaces)
31
Q

how to name alkenes and alkynes?

A
  1. Find the parent chain. It MUST contain the multiple bond.
    – Ifthe bond is a double, the suffix for the parent chain will be ‐ene
    – If the bond is a triple, the suffix for the parent chain will be –yne
  2. Count carbon atoms so that the multiple bond will be on the lowest possible number. Indicate the number that the multiple bond falls on directly before the suffix
  3. name branches as usual
  4. if there is more then one double bond indicate both numbers where the double bond is formed, and change the suffix to –diene
32
Q

what is an isomer and how to identify?

A

Compound with ONLY the same molecular formula but different structures
– They will have different chemical and physical properties–based on their different structures

33
Q

what is benzene?

A
  • C6H6
  • unreactive
  • aromatic
  • ring with alternating double bonds
  • when naming if it not the parent chain it is given the branch name “phenyl”
34
Q

how to name alkyl halides?

A

name like a regular branch but drop the ending of the halogen and replace with -o

35
Q

what is a carboxcylic acid and how to name?

A

A carboxyl group is composed of a carbon atom double bonded to an oxygen atom and bonded to a hydroxyl group (‐COOH)

  • always at the end of the parent chain
    1. Name the parent alkane
    2. Replace the –e at the end of the name of than parent alkane with –oic acid
    3. The carbon atoms of the carboxyl group is always given position number 1. Name and number the branches that are attached to the compound.
36
Q

what is an ester and how to name?

A

The reaction between a carboxylic acid and an alcohol produces
an ester molecule and a molecule of water
– This reaction is known as acondensation or esterification reaction
The ester functional group –COO– is similar to that of a carboxylic acid, except that the H atom of the carboxyl group has been replaced by a hydrocarbon branch.
– Esters are responsible for natural and artificial fragrance and flavourings in plants and fruits.

butanoic acid + ethanol ==> ethyl butanoate + water

37
Q

order of boiling point for simple hydrocarbons? other properties?

A

alkyl halides – alkanes – alkenes – alkynes

  • boiling point goes up with number of carbons
  • more branching = less london dispersion, lower boiling point
  • all non polar, insoluble in water
38
Q

order of boiling point for hydrocarbon derivatives?

A

alcohols – carboxylic acids – esters

  • high BP caused by Hbonds
  • same order for solubility
  • these 3 are higher then simple hydrocarbons
39
Q

what is an addition reaction?

A

reaction of alkenes and alkynes with hydrogen gas, a halogen compound, or a hydrogen halide compound
occurs fast
hydrogenation
alkene/kyne + H2 –> alkane

40
Q

what is a subsititution reaction?

A

the breaking of a C–H bond in an alkane or aromatic ring and replacing it with another atom
often substitutes a halogen for a hydrogen
no change in saturation
occurs slowly
alkane + halide –> organic halide + hydrogenhalide

41
Q

what is an elimination reaction?

A

eliminating atoms or groups of atoms d
decreasing saturation
alkane craked into alkene by removing hydrogen gas
removing water from ethanol to make ethene
Alkyl halide reacts with a hydroxide ion (OH‐) to produce an alkene (dehydrohalogenation–removes a hydrogen and halogen atom)

42
Q

what is addition polymerization?

A

always results in one product, the polymer
• Requires unsaturated hydrocarbon monomers and bond saturation occurs when the polymer is made

ethene (double bond) –> polyethene (single bonded polymer)

43
Q

what is condensation polymerizaton?

A

Monomers combine to form a polymer and a bi‐product.
Each time a bond forms between monomers, small molecules,
such as water, ammonia, or HCl are “condensed” out.
• For condensation polymerization to occur, monomers must be bifunctional, meaning they have at least two functional groups.
• If they only had one functional group, then only one bond would
form.

44
Q

what is polyester?

A

When a carboxylic acid reacts with an alcohol in an esterification
reaction, a water molecule is eliminated and a single ester molecule is formed
• This esterification reaction can be repeated so many esters are
joined in a long chain… a polyester
– This is created using a dicarboxylic acid (an acid with a carboxyl group at each end) and a diol (an alcohol with a hydroxyl group at each end)
– The ester linkages are formed end to end between alternating acid and alcohol molecules

45
Q

what is a fractional distillation tower?

A

A fractional distallation tower contains trays positioned at various
levels.
• Heated crude oil enters near the bottom of the tower.
• The bottom is kept hot, and the temperature gradually decreases toward the top of the tower.
• As compounds cool to their boiling point, they condense in the cooler trays. The streams of liquid (called fractions) are withdrawn from the tower at various heights along the tower

46
Q

what is an alcohol and how to name?

A
  1. Find the longest chain containing the hydroxy group (OH). If there is a chain with more carbons than the one containing the OH group it will be the subsitutent.
  2. Give the OH on the lowest possible number for the chain.
  3. When naming a cyclic structure, the -OH is assumed to be on the first carbon
  4. When multiple -OH groups are on the cyclic structure, number the carbons on which the -OH groups reside.
  5. Remove the final e from the parent alkane chain and add -ol. 6.When multiple alcohols are present use di, tri, et.c before the ol, after the parent name. ex. 2,3-hexandiol. If a carbonyl group is present, the -OH group is named with the prefix “hydroxy,” with the carbonyl group attached to the parent chain name so that it ends with -al or -one.

Biology 30 (2 decks)

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