Chapter 3: The Mole - The Central Unit of Chemistry Flashcards

1
Q

object with more mass contains _____ particles, compared to an object of less mass

A

larger

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2
Q

def: a ration of one object’s mass to that of another object

A

relative mass

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3
Q

what is the one essential criteria for determining the relative mass between two objects?

A

both groups of objects contain the same number of objects

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4
Q

what assumptions are we making when we determine relative mass?

A

that all the objects in one group are identical to each other in mass

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5
Q

def: all samples of a given compound contain the same elemental composition by mass, meaning their elements are always present in a fixed ration

A

law of constant composition

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6
Q

who presented the theory that “atoms of different elements combine in simple whole-number ratios to form compounds”?

A

john dalton

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7
Q

what was wrong with Dalton’s theory that atoms combine in simple whole number ratios?

A

he assumed that elements ALWAYS combine in the simplest possible ratio

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8
Q

what were two parts to Dalton’s atomic theory?

A
  1. atoms of a given element are identical to each other, but different from those of other elements
  2. atoms of different elements combine in a simple whole-number ratio to from compounds
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9
Q

you can determine absolute values directly, while relative values require _______________

A

comparing to a second value

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10
Q

what element did Dalton assign the atomic mass unit to?

A

hydrogen as it is the least massive

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11
Q

def: a dimensionless ratio of the average mass of an element’s atoms compared to an agreed upon and consistent reference

A

relative atomic mass

Ar

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12
Q

what is our current reference for relative atomic mass?

A

the carbon-12 atom

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13
Q

what did Cannizzaro’s paper clear up?

A

that some elements don’t exist as individual atoms when alone, they exist as diatomic molecules

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14
Q

def: seven elements whose particles are homonuclear diatomic molecules, rather than individual atoms

A

diatomic element

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15
Q

def: describes a molecule formed of identical atoms

A

homonuclear

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16
Q

def: describes a molecule formed of different atoms

A

heteronuclear

17
Q

def: an SI unit for the amount of stuff, or quantity, equal to the number of atoms in exactly 12 g of pure carbon-12

A

mole

18
Q

def: the number of things in one mole, defined by 6.02 X 10^23

A

Avogradro’s Constant

19
Q

def: the mass of one mole of substance, whether its particles are atoms, ions or molecules

A

molar mass

20
Q

the relative atomic masses listed on the periodic table are the ________ for the elemnts

A

molar masses

21
Q

the molar mass of compounds is the ___ of all the molar

masses of the atoms that make up the compound

A

sum

22
Q

we cannot convert from ______ to ______ in one step

A

mass to number of particles

23
Q

def: the calculation of relative quantities between two substances, be they elements within a compound or some mix of reactants and products in a chemical reaction

A

stoichiometry

24
Q

what are the two types of stoichiometry?

A

composition and reaction

25
Q

def: the ration between the moles of two substances, from either a chemical formula of balanced chemical equation

A

mole ratio