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My Packs: UWO (CHEM 1301) > Chapter 1: 1.1 Atoms, Molecules, and Moles > Flashcards

Chapter 1: 1.1 Atoms, Molecules, and Moles Flashcards

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1
Q

Atoms consist of:

A

Protons
Neutrons
Electrons

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2
Q

Charge of proton

A

Positive

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3
Q

Charge of neutron

A

Electrically neutral

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4
Q

Charge of electron

A

Negative

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5
Q

Do protons and neutrons have the same mass?

A

Almost the same mass

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6
Q

The mass of an electron is only ______th of the mass of a proton or a neutron

A

1/1836

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7
Q

Atomic number

A

The number of protons in an atomic nucleus

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8
Q

Where are protons and neutrons found?

A

In the atom’s nucleus

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9
Q

Mass number

A

The total number of protons and neutrons in an atom

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10
Q

Atomic mass unit

A

The chemical unit of atomic mass, also known as Dalton

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11
Q

Define 1 u (atomic mass unit)

A

Exactly 1/12 of the mass of a C-12 atom

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12
Q

What is Dalton denoted by?

A

“Da”

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13
Q

Isotopes

A

Atoms with the same number of protons but different numbers of neutrons

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14
Q

Isotopes have the same ____ number but a different ____ number

A

Same atomic number
Different mass number

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15
Q

Isotopic abundance

A

The percent by number of each of the isotopes of an element

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16
Q

Average atomic mass

A

The average of the masses of all of the isotopes of that element

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17
Q

Why is it that the atomic mass an element less than the atomic mass of the nucleus?

A

When protons and neutrons combine to form a nucleus, some of their total mass is converted into energy

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18
Q

What is the difference between the atomic mass of an element and the atomic mass of the nucleus known as?

A

Mass Defect

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19
Q

Neutral atom

A

Atoms that have an equal number of protons and electrons

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20
Q

Cation

A

Atom with a positive charge

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21
Q

Anion

A

Atom with a negative charge

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22
Q

What are ions of molecules called?

A

Molecular (or complex) ions

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23
Q

Compound

A

A molecule containing atoms of more than one element

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24
Q

Is O2 a compound?

A

No

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25
Q

Diatomic molecule

A

A molecule with only two atoms (such as O2)

26
Q

Polyatomic molecule

A

A molecule with more than two atoms (such as H2O)

27
Q

Empirical formula

A

Represents the simplest ratio of the numbers of atoms in a molecule

28
Q

What is the empirical formula of glucose (C6H12O6)?

A

CH2O

29
Q

Define a mole

A

The number of atoms contained in exactly 12 grams of pure carbon-12

30
Q

What is the symbol for number of moles

A

n

31
Q

Determine the number of individual atoms, molecules, or ions in a sample

A

Moles * Avogadro’s number

32
Q

What is the number of atoms contained in exactly 12 grams of pure carbon-12 known as?

A

Avogadro’s number
(6.02 * 10^23)

33
Q

1 mole of carbon-12 = __ grams

A

12 grams of carbon-12

34
Q

If one mole of carbon-12 atoms has a mass of exactly 12 g, what is the mass in grams per mole for carbon-12?

A

12 grams per mole

35
Q

Unit used for the mass of one atom

A

u

36
Q

Unit used for the mass of a mole of atoms

A

g

37
Q

Molecular mass

A

The mass of one molecule computed as the sum of atomic masses of all the atoms in the molecule

38
Q

What is molecular mass usually expressed in?

A

Atomic mass units

39
Q

Molar mass (MM)

A

The mass of one mole of molecules

40
Q

What is the unit for molar mass?

A

Grams per mole

41
Q

Formula of mass percent

A

(Mass of one species / Total mass of sample) * 100%

42
Q

Mass percent of a species cannot exceed ____

A

Cannot exceed 100%

43
Q

Sum of mass percents must add up to:

A

100%

43
Q

Formula of mole fraction

A

(Number of moles of one species / Total number of moles)

44
Q

Formula of Mole percent

A

Mole fraction * 100%

45
Q

What is used to represent to mole fraction of an element or compound?

A

The symbol X with a subscript of the element or compound

46
Q

Solution

A

A homogeneous mixture of two or more substances

47
Q

Solute

A

Substance Dissolved

48
Q

Solvent

A

Dissolving substance

49
Q

Molarity

A

The number of moles of solute in one litre of the solution

50
Q

Symbol for molarity

A

M

51
Q

Formula for molarity

A

Amount of solute / Volume of solution

or

M = n/V

52
Q

True or False:
When calculating molarity, volume can be calculated using millilitres or litres

A

False, when calculating molarity, volume can only be calculated using liters

53
Q

Dilution

A

The process of reducing the concentration of a solution, either by adding the solvent or buy adding another solution

54
Q

Provided no chemical reaction takes place, when a solution is diluted with the solvent, or mixed with a solution of another substance, does the number of moles of solute change?

A

No

55
Q

Define a chemical reaction

A

A process in which one set of substances, called reactants, is converted to a new set of substances, called products

56
Q

What is the literal meaning of stoichiometry?

A

“The measurement of elements”

57
Q

Theoretical yield

A

The expected amounts of products (can be calculated)

58
Q

Actual yield

A

The amount of product collected

59
Q

Percent yield

A

The ratio of the actual yield to the theoretical yield

60
Q

True or False:
Actual and theoretical yields can be expressed in different units when calculating percent yield

A

False, they must both be expressed in the same units (moles or masses)

61
Q

Limiting reagant

A

The reagent whose amount (number of moles) is insufficient to react completely with all the other reagents, as determined by the stoichiometry of the reaction

My Packs: UWO (CHEM 1301) (17 decks)

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