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Princeton MCAT Chemistry > Fundamentals > Flashcards

Fundamentals Flashcards

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1
Q

What is an amp?

A

A unit of measurement for electricity

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2
Q

1 Mega = __________

A

10^6 (MegaBYTE)

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3
Q

What is the relationship between liters and cm?

A

1L = 1000cm^3 (both units of volume)

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4
Q

1m^3 = ?

A

1 m^3 = 1000L

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5
Q

1mL = ____ cm^3 = ___cc

A

1ml = 1 cm3 = 1 cc

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6
Q

Angstrom is equal to ?

A

1 A = 1.0 ^ -10 m

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7
Q

Why is the angstrom useful as a unit of measurement?

A

It the right range for atomic radius and bond length

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8
Q

What is the range for atomic radii and bond length in angstrom?

A

1 to 3 Angstrom

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9
Q

By how many orders of magnitude is a centimeter longer than an angstrom?

A

1 cm = 10^ -2 m 1 Angstrom = 1E-10 m the difference is 8 orders of magnitude or factor of 8.

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10
Q

What are the two common units of density?

A

kg/m3 or g/cm3

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11
Q

What is the conversion between kg/m3 to g/cm3?

A

kg/m3 to g/cm3 divide by 1000 (Going from Larger unit to smaller duh)

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12
Q

What is the conversion between g/cm3 to kg/m3?

A

multiply by 1000

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13
Q

What is the density of water (g/cm3)?

A

1g/cm3

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14
Q

What is the density of water (kg/m3)?

A

1000kg/m3

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15
Q

What is a molecular formula?

A

A molecular formula tells us the identity and the number of each atom in a molecule ex. H20

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16
Q

A molecule is composed of ________

A

A molecule is formed when two or more elements are chemically joined (they can be the same or different)

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17
Q

What makes a compound?

A

Compounds are a type of molecule. A molecule that contains at least two different elements.

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18
Q

Are all compounds molecules?

A

Yes all compounds are molecules.

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19
Q

Are all molecules compounds?

A

No because O2 or H2 are molecules but can’t be compounds.

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20
Q

What is an empirical formula?

A

Method to describes the Numerical Proportions of atoms by using the smallest whole number to describe the same ratio of the atoms as in the molecular formula.

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21
Q

What is a chemical formula?

A

Method of expressing the exact number of atoms in a molecule.

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22
Q

If we know the chemical formula and we use the atomic weights listed on the period table what can we automatically figure out about the molecule overall?

A

The formula weight.

23
Q

What is formula weight?

A

The sum of the atomic weights of all the atoms in the molecule.

24
Q

What is the unit for atomic weight(mass)?

A

atomic mass unit (amu)

25
Q

One atomic unit has been established to be equal to?

A

1/12 of the mass (g) of an atom of Carbon-12.

Carbon has 6 proton and 6 neutron. In grams this is 12*1.66E-24 grams = 2.0E-23 grams

26
Q

The masses listed on the period table are an average of?

A

the weight average of the atomic mass units (amu) of all the naturally occurring isotopes of each element based on their abundance.

27
Q

What is molecular weight?

A

Molecular weight is commonly used to describe the atomic mass of a molecule (it is the same as formula weight)

28
Q

When is molecular weight used vs formula weight?

A

Molecular weight is used for molecules while formula weight is used for ionic compounds.

29
Q

What is the mole?

A

The mole is a unit that relates atomic mass unit to grams. It is based on the atomic mass unit.

30
Q

1 mole is = ?

A

1 mole = 6.022 ^ 23 atoms, molecules, ions, photon, electrons

31
Q

what is the number of carbon-12 atoms in a sample mass of 12 grams?

A

6.022^23

32
Q

12 g of Carbon 12 =

A

1 mole of Carbon = 6.022E23 atoms= 12 amu

33
Q

Molecule’s percent mass composition cab be determined using what two formulas?

A

Empirical and molecular formula

34
Q

Quickly Determine the percent of Carbon in C4H4N2?

A

2(12)/( 2x12 + 2x1 + 14) = 24/40 = .6 = 60%

35
Q

Determine the empirical formula for a compound that contains 70% Iron and 30 % Oxygen?

A 
70% = 70 grams of Iron
30 % = 30 grams of Oxygen
Convert the grams to moles:
70 grams/55.8 g per mole = 5/4 = 1.25 moles
30/16 = 15/8 
Determine the ratio of Iron to Oxygen
 (5/4) moles/ (15/8) moles = 2/3

Ratio of Iron to Oxygen is 2:3

Fe 2 O 3

36
Q

What is Molarity?

A

moles of solute/ liters of solution

37
Q

What is mole fraction?

A

The mole fraction (S)= number of moles of substance S / total moles in the solution

38
Q

When is mole fractions used?

A

When more than one solute is present in solution and is most commonly used when discussing the composition of a mixture of gases.

39
Q

The mass of a proton

A

1.66x10-24g

40
Q

The mass of a neutron

A

1.66x10-24g

41
Q

1 amu = ____ grams

A

1.66E10-24g (mass of proton/neutron)

42
Q

In a chemical equation the Law of Conservation of Mass states that what must be true about the chemical equation?

A

The number of atoms on the reactants must equal the number of atoms on the products because the amount of matter (mass) does not change in a chemical reaction.

43
Q

In a chemical equation the stoichiometric coefficients provide what information ?

A

The stoichiometric coefficients tells us the ratios of moles or molecules involved in the chemical equation not the ratios of mass.

44
Q

How do we assign oxidation states?

A

Based on who owns the electrons(not share that is formal charge) in the molecule which is determined base on the affinity of the atoms towards electrons.

45
Q

What are the main rules for assigning oxidation states to atoms?

A
  1. The oxidation of any element in its standard state is 0
  2. Sum of the oxidation states of each atom in a molecule that is in its neutral state must sum up to 0.
  3. Group I atoms are assigned an oxidation state of + 1
  4. Group II atoms are assigned an oxidation state of +2
  5. Group VII has an oxidation state of -1.
  6. Hydrogen has an oxidation state of +1 when bonded to something more electronegative than carbon and - 1 when bonded to something less electronegative than carbon and 0 when bonded to Carbon.
  7. Oxygen usually -2 except in peroxides or other compounds where it is forced to only take one electron since such as H2O2 or Na2O2 (oxdiation state of -1)
    It can also be found at an oxdiation state of 0 if element.
    It can have an oxidation state of +2 when it is not the most electronegative atom such as F2O.
46
Q

What is oxidation state of an element in its standard state?

A
  1. The oxidation of any element in its standard state is 0
47
Q

Sum of the oxidation states of each atom in a neutral molecule must equal?

A

0

48
Q

Group I and II atoms have what oxidation states (except for Hydrogen)

A

+1 (Group 1) and +2 (group 2)

49
Q

Group VII atoms have what oxidation state?

A

They have an oxidation state of -1

50
Q

Oxygen has what oxidation states?

A
  • 2 generally except for
    1. when found in peroxides or group 1 metals then it adopts -1 charge
    2. when bound to atom more electronegative than it is (Flouride) then it picks up +2 charge.
51
Q

what oxidation state does hydrogen have?

A

Hydrogen will pick up - 1 charge when bound to atoms less electronegative than Carbon and + 1 charge when bound to atoms more electronegative then Caron and charge of 0 when bound to Carbon.

52
Q

What is the order of electronegativity of some important elements?

A

FONClBrISCH (pronounced fawn-cull-brish) with flouride most electronegative and H least

53
Q

What is the oxidation state of Fe3O4?

A

In this example Oxygen has -2 (-8 total) and Iron has to be (+8/3). We can have fractional charges. Two atoms of iron will have +3 charge while one will have +2.

Princeton MCAT Chemistry (2 decks)

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