To calculate the number of atoms present in 2.0 mol of an element, you would

multiply Avogadro's number of atoms per mole by 2.0 mole

To determine the mass in grams of an atom of any element, you would

divide mass of a mole of element by Avogadro's number

The molar mass of an element is numerically equal to

the element's average atomic mass

The average atomic mass of an element is

the weighted average of all naturally occurring isotopes of the element

According to law of definite proportions, any two samples of KCl will have

the same elements in the same proportions by mass

Which of the following is not one of the five principles of Dalton's theory?

all atoms have similar physical and chemical properties

Atomic mass of 1 atom of Carbon = 12 amu. Atomic mass of 1 atom of oxygen is 16 amu. CO = 16 O & 12 C. CO2 = 32 O & 12 C

ratio of oxygen to carbon is 2:1

According to law of conservation of mass: sodium, hydrogen, and oxygen react to form a compound. Mass will be

equal to the sum of the masses of the reactants

Rutherford's gold-foil experiment led him to conclude that

a dense region of positive charge existed somewhere in the atom

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Chemistry Chapter 3: Structure of an Atom

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Answers

1
The least massive particle in an atom is the
none of the above
electron
neutron
proton
2
To calculate the number of atoms present in 2.0 mol of an element, you would
multiply Avogadro's number of atoms per mole by 2.0 mole
divide Avogadro's number of atoms per mole by 2.0 mole
subtract Avogardro's number of atoms per mole from 2.0 mole
add Avogadro's number of atoms per mole to 2.0 mole
3
To determine the mass in grams of an atom of any element, you would
multiply mass of a mole of element by Avogadro's number
add the mass of a mole of element to Avogadro's number
divide mass of a mole of element by Avogadro's number
subtract the mass of a mole of element to Avogadro's number
4
What is the mass of 3.56 mol of glucose, C₆H₁₂O₆? (molar mass is 180.18 g/mol)
.0198 g
641 g
2.14 x 1024 g
50.6 g
5
The molar mass of an element is numerically equal to
the element's average atomic number
the percentage composition of the element by mass
the number of electrons possessed by an element
the element's average atomic mass
6
Compared with a mole of lead atoms, a mole of iron atoms
has the same number of atoms
has more atoms
cannot be determined because iron is magnetic
has fewer atoms
7
Thomson's experiment showed that the charge to mass ratio of electrons was
less with noble gases than for other gases
the same in all gases
greater with noble gases than for other gases
dependent on the element's atomic mass
8
The ancient Greek natural philosopher who first proposed the notion of the atom was
Plato
Democritus
Socrates
Aristotle
9
The molecular mass of CO₂ is 44.01 amu. What is the mass of 2.0 mol
88.02 amu
44.01 amu
44.01 g
88.02 g
10
The units of molar mass are
mol/g
g/mol
amu/g
amu/mol
11
Which feature of Dalton's atomic theory is different form modern atomic theory?
atoms cannot be subdivided
atoms cannot be rearranged in chemical reactions
atoms combine in whole-number ratios
atoms cannot be destroyed
12
The atomic symbol for beryllium, ⁹₄Be, indicates that the
atomic number is equal to 9 - 4
atomic number is 4
atomic number is 9
mass number is 4
13
The average atomic mass of an element is
the same as the atomic number of the element
the sum of the number of neutrons and protons in a an atom
the weighted average of all naturally occurring isotopes of the element
the mass of one isotope of the element
14
How many moles of sodium hydroxide, NaOH, are in a 35.65 h sample of NaOH? (molar mass is 40.01 g/mol)
5.366 x 1023 mol
1.122 mol
1426 mol
.8910 mol
15
According to law of definite proportions, any two samples of KCl will have
the same elements in the same proportions by mass
the same mass
different densities
slightly different molecular structures but same 2 elements
16
Protons are bound together by
magnetic forces
electric forces
gravitational forces
strong nuclear forces
17
Which of the following is not one of the five principles of Dalton's theory?
Atoms of diff elements combine in whole number ratios to form compounds
Chemical reactions consist: combination, separation or rearranging of atoms
all matter is made indivisible, indestructible atoms
all atoms have similar physical and chemical properties
18
Atomic mass of 1 atom of Carbon = 12 amu. Atomic mass of 1 atom of oxygen is 16 amu. CO = 16 O & 12 C. CO₂= 32 O & 12 C
ratio of oxygen to carbon is 1:2
ratio of oxygen to carbon is 8:3
ratio of oxygen to carbon is 2:1
ratio of oxygen to carbon is 1:1
19
The most massive particle in an atom is the
neutron
proton
none of the above
electron
20
Which of the following is NOT equal to 1.00 mol of carbon-12?
12.0 g of carbon
6.022 x 1023 atoms
both b and c
6.0 g of carbon
21
According to law of conservation of mass: sodium, hydrogen, and oxygen react to form a compound. Mass will be
either less than or equal to the sum of the masses of the reactants
less than the sum of the masses of the reactants
equal to the sum of the masses of the reactants
greater than the sum of the masses of the reactants
22
An atom of potassium has 19 protons and 20 neutrons. Its mass number is
19
39
20
9
23
Rutherford's gold-foil experiment led him to conclude that
a dense region of positive charge existed somewhere in the atom
light was emitted by electrons returning to ground state
Thomson's plum pudding model was accurate
alpha particles were a poor choice for a bombardment material
24
The word atom means
charged
indestructable
indivisible
energetic
25
Neutral atoms contain equal numbers of
electrons and neutrons
protons and neutrons
protons, electrons, and neutrons
protons and electrons

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