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

The molar mass of an element is numerically equal to

the element's average atomic mass

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

the same elements in the same proportions by mass

The law of conservation of mass states that when Na, H, and O form a compound, the mass will be

equal to the sum of the masses of the reactants

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

All matter is made of indivisible, indestructible atoms

The average atomic mass of an element is

the weighted average of all natural isotopes of the element

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

a dense region of positive charge existed in the atom

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

divide the mass of a mole of an element by Avogadro’s number

studbud

Chapter 3

25 termsStudBud Administration447 plays

Chapter Three

Flashcards25 cardsFPractice quizPHost liveL

Questions 25

Answers

1
The atomic symbol for beryllium, ⁹₄Be , indicates that the
atomic number is 4
mass number is 4
atomic number is equal to 9 - 4
atomic number is 9
2
Compared with a mole of lead atoms, a mole of iron atoms
cannot be determined because iron is magnetic
has fewer atoms
has the same number of atoms
has more atoms
3
To calculate the number of atoms present in 2.0 mol of an element, you would
subtract Avogadro’s number of atoms per mole from 2.0 mole
add Avogadro’s number of atoms per mole to 2.0 mole
multiply Avogadro’s number of atoms per mole by 2.0 mole
divide Avogadro’s number of atoms per mole by 2.0 mole
4
Which feature of Dalton’s atomic theory is different from modern atomic theory?
Atoms cannot be rearranged in chemical reactions
Atoms cannot be subdivided
Atoms combine in whole-number ratios
Atoms cannot be destroyed
5
The molar mass of an element is numerically equal to
the number of electrons possessed by an element
the % composition of the element by mass
the element's average atomic number
the element's average atomic mass
6
The molecular mass of CO₂ is 44.01 u. What is the mass of 2.0 mol of CO₂?
44.01 g
88.02 g
44.01 u
88.02 u
7
Which of the following is not equal to 1.00 mol of carbon 12?
6.0 g of carbon
12g of carbon and 6 g of carbon
6.022 x 1023 carbon atoms
12.0 g of carbon
8
According to the law of definite proportions, any two samples of KCl will have
different molecular structures but the same two elements
the same elements in the same proportions by mass
different densities
the same mass
9
Protons are bound together by
electric forces
strong nuclear forces
magnetic forces
gravitational forces
10
The least massive particle in an atom is
the electron
your mother
the proton
the neutron
11
Neutral atoms contain equal numbers of
protons and electrons
protons and neutrons
electrons and neutrons
protons, electrons, and neutrons
12
The law of conservation of mass states that when Na, H, and O form a compound, the mass will be
less than the sum of the masses of the reactants
greater than the sum of the masses of the reactants
less than or equal to the sum of the masses of the reactants
equal to the sum of the masses of the reactants
13
The ancient Greek natural philosopher that first proposed the notion of the atom was
Democritus
Socrates
Aristotle
Plato
14
The word "atom" means
charged
indivisible
energetic
indestructible
15
The units of molar mass are
amu/g
amu/mol
mol/g
g/mol
16
Which of the following is not one of the five principles of Dalton’s theory?
Chemical reactions consist of the rearrangement of atoms
All atoms have similar physical and chemical properties
All matter is made of indivisible, indestructible atoms
Atoms of different elements combine in simple, whole-numbers
17
The average atomic mass of an element is
the sum of the number of neutrons and protons in an atom
the same as the atomic number of the element
the weighted average of all natural isotopes of the element
the mass of one isotope of the element
18
How many moles of NaOH are in a 35.65 g sample of NaOH? The molar mass of NaOH is 40.01 g/mol.
5.366 x 1023 mol
1.122 mol
0.8910 mol
1426 mol
19
The ratio of the mass of oxygen in CO₂ to the mass of oxygen in CO is
2:1
8:3
1:2
1:1
20
Rutherford's gold-foil experiment led him to conclude that
Thomson's plum pudding model of the atom was accurate
light was emitted by electrons returning to ground state
a dense region of positive charge existed in the atom
alpha particles were a poor choice for bombardment
21
An atom of potassium has 19 protons and 20 neutrons. Its mass number is
20
9
39
19
22
To determine the mass in grams of an atom of any element, you would
divide the mass of a mole of an element by Avogadro’s number
add the mass of a mole of the element to Avogadro’s number
multiply the mass of a mole of the element by Avogadro’s #
subtract the mass of a mole of an element from Avogadro’s #
23
The most massive particle in an atom is
the electron
the neutron
Your daddy
the proton
24
What is the mass of 3.56 mol of glucose, C₆H₁₂O₆? (The molar mass of C₆H₁₂O₆ is 180.18 g/mol.)
50.6 g
641 g
2.14 x 1024 g
0.0198 g
25
Thomson’s experiment showed that the charge-to-mass ratio of electrons was
the same in all gases
dependent on the element's atomic mass
less with noble gases than for other gases
greater with noble gases than for other gases

Chapter 3 Flashcards | StudBud