Deck 2: The Structure of Matter

Question 1

A positively charged nucleus surrounded by negatively charged electrons in well-defined orbits is the ___________ model of the atom.

A) Bohr
B) Thomson
C) Rutherford
D) Dalton

Answer 1

Bohr

Question 2

An atom in a normal state has an electrical charge of _______.

A) one
B) zero
C) positive
D) negative

Answer 2

zero

Question 3

Two identical atoms which exist at different energy states are called ____________.

A) isotopes
B) isomers
C) isotones
D) isobars

Answer 3

isomers

Question 4

The atomic number of an element is symbolized by the letter _____.

A) A
B) X
C) Z
D) n

Question 5

The term "atom" was first used by the ___________.

A) Ethiopians
B) British
C) Greeks
D) Romans

Question 6

An atom that loses or gains one or more electrons is a(n) ________.

A) ion
B) molecule
C) isotope
D) isomer

Question 7

The first person to describe an element as being composed of identical atoms was __________.

A) J. J. Thomson
B) John Dalton
C) Dmitri Mendeleev
D) Niels Bohr

Question 8

The maximum number of electrons that can exist in an electron shell is calculated with the formula _____.

A) 2n
B) 2n2
C) 2/n
D) 2/n2

Question 9

The shell number of an atom is called the ___________________.

A) alpha particle
B) chemical element
C) principal quantum number
D) half-life number

Question 10

A neutral atom has the same number of _________ and electrons.

A) quarks
B) neutrinos
C) neutrons
D) protons

Question 11

The innermost electron shell is symbolized by the letter _____.

A) J
B) K
C) L
D) M

Question 12

Aluminum has an atomic number of 13. How many protons does it have?

A) 13
B) 26
C) 27
D) None of the above

Question 13

Rutherford's experiments in 1911 showed that the atom was composed of _________________.

A) electrons with well-defined orbits
B) a nucleus with an electron cloud
C) electrified plum pudding
D) a ball of hooks and eyes

Question 14

The binding energies, or energy levels, of electrons are represented by their ___________.

A) atomic numbers
B) atomic mass units
C) shells
D) isotopes

Question 15

When an atom has the same number of protons as another, but a different number of neutrons, it is called an __________.

A) isomer
B) isobar
C) isotone
D) isotope

Question 16

The chemical element is determined by the number of __________ in the atom.

A) protons
B) electrons
C) neutrons
D) nucleons

Question 17

The smallest particle that has all the properties of an element is a(n) __________.

A) neutron
B) proton
C) electron
D) atom

Question 18

When atoms of various elements combine, they form __________.

A) isotopes
B) compounds
C) molecules
D) ions

Question 19

The periodic table of the elements was developed by __________ in the late 19th century.

A) Bohr
B) Rutherford
C) Mendeleev
D) Roentgen

Question 20

What are the fundamental particles of an atom?

A) Quark, positron, negatron
B) Nucleon, electron, proton
C) Proton, neutron, quark
D) Proton, electron, neutron

Question 21

The atomic number of molybdenum is 42 and the atomic mass number is 98. How many neutrons does it have?

A) 42
B) 98
C) 21
D) 56

Question 22

A chemical compound is any quantity of _______________.

A) one type of atom
B) one type of molecule
C) two types of molecules
D) two or more types of atoms

Question 23

The only difference between x-rays and gamma rays is their _________.

A) energy
B) size
C) origin
D) name

Question 24

The __________ is the least penetrating form of ionizing radiation.

A) beta particle
B) x-ray
C) gamma ray
D) alpha particle

Question 25

During beta emission, an atom releases ___________.

A) electrons
B) positrons
C) protons
D) neutrons