From Science Matters by Robert H. Hazen and James Trefil, Doubleday, 1991
A pure substance that can't be broken down by chemical means; an atom for which you know the exact number of protons:
element
proton
neutron
electron
nucleus
Breaking down a substance by burning or immersion in acid is by using a ( ) means.
chemical
physical
nuclear
biological
The smallest particle any substance can be broken down into by chemical means:
atom
element
proton
electron
neutron
The heavy central part of every atom; contains protons and neutrons
nucleus
electron
element
isotope
ion
A positively charged particle in the nucleus; the number of which distinquishes one element from another:
proton
atom
neutron
electron
An electrically neutral particle in the nucleus:
neutron
proton
electron
ion
isotope
An electrically negative particle that orbits the nucleus:
electron
proton
neutron
isotope
ion
An atom for which you know both the exact number of neutrons and the number of protons:
isotope
electron
element
ion
Different isotopes of a given element have:
the same chemical properties
different numbers of neutrons
the same numbers of neutrons
different chemical properties
different numbers of protons
An atom that has gained or lost electrons, and hence has an electrical charge:
ion
isotope
nucleus
element
The subatomic particles that make up an atom include:
proton, neutron, electron
proton, neutron, ion
proton, nucleus, electron
isotope, neutron, element
The diversity of different kinds of atoms, such as hydrogen, copper, sulfur, and uranium:
chemical elements
elements
ions
isotopes
orbits
Common chemicals consist of precise ratios of:
elements
protons
electrons
neutrons
isotopes
The orginal idea of the atom is usually associated with:
the philospher Democritus
a Greek who lived in the fifth century B.C.
John Dalton
an English chemist (1766-1844)
Albert Einstein
The modern notion of the atom came from:
the English chemist John Dalton (1766-1844)
the results of laboratory experiments
philosophical reasoning
the Greek Democritus
Albert Einstein
Brownian motion
When a small particle such as a grain of pollen is suspended in a liquid and observed under a microscope, it is seen to move around in a random, erratic path. This phenomenon is called:
Brownian motion
Einstein motion
quark motion
Dalton motion
Substances that could not be broken down at all, including oxygen, gold, sulfur, and iron, Dalton called:
elements
minerals
nobel
isotopes
That suspended particles move because of collisions with atoms was used by Einstein to:
argue that atoms must be real
define Brownian motion
obtain photographs of individual atoms
demonstrate quarks
"Photographs" of individual atoms can now be taken with the ( ) microscope.
scanning tunneling
electron
light
atom
infra-red
The massive central nucleus of an atom surrounded by smaller electrons, and the sun surrounded by planets represent:
an analogy
a similarity
systems held together by the same forces
systems held together by gravity
systems held together by electrical forces
An atom has a neutral charge do to:
the positive nucleus and the negative electrons
the positive protons and the negative electrons
the positive charges on neutrons and protons
the negative charges on nucleus and electrons
neutral gravitational attraction
Some 99.9 percent of an atom's mass is:
located in the nucleus
composed of protons and neutrons
made up of protons
made up of neutrons
located in orbiting electrons
The number of protons determines;
how an atom will behave
the type of chemical element
the atomic weight
the isotope
Each chemical element is defined exclusively by its number of protons--the so-called:
atomic number
atomic weight
atomic charge
The naturally occurring elements are numbered from 1 (hydrogen) to:
94 (plutonium)
95 (americium)
96 (curium)
93 (neptunium)
98 (californium)
Neutrons weigh roughly the same as protons but:
lack an electrical charge
have little effect on the way one atom interacts with another
are smaller than protons
have little effect on the atomic mass
have little effect on holding the nucleus together
Scientists customarily denote an isotope by giving the combined total of:
protons and neutrons
the atomic mass
protons and electrons
neutrons and electrons
subatomic particles
atomic number and atomic mass
An electron simply disappears from one orbit and reappears in another without traversing the space in between by means of:
a quantum leap
gaining or losing energy
emitting light to reach a higher orbit
absorbing energy to slow down to a lower orbit
This picture, in which electrons shuttle back and forth between allowed orbits as they absorb and emit energy, is called:
the Bohr atom
the periodic table
the Bohr orbit
Brownian motion
Substances that make up the pieces of more complex materials but which are themselves irreducible, chemists termed:
elements
isotopes
ions
subatomic particles
The names of elements are customarily represented:
by a one- or two-letter abbreviation
as Ca for calcium
as Hy for hydrogen
by a one- or two-letter Latin symbol
Elements in the same column in the periodic table:
enter into similar reactions
combine to form similar compounds
have the same number of orbits for electrons
have the same atomic mass
have the same number of neutrons
A molecule composed of more than one type of atom or element:
compound
isotope
nucleus
diatomic
The periodic table of the elements was first written down:
by the Russian scientist Dmitri Mendeleyev in 1869
with two holes corresponding to germanium and scandium
by the German scientist Albert Einstein in 1905
by the English chemist John Dalton in 1840
by knowing that a ranking of the elements in increasing order of weight had something to do with their chemical properties
Elements in the top row of the periodic table have electrons:
in one orbit only
in an orbit that can hold two electrons
in two orbits
in three orbits
in orbits that can hold 8 electrons
Elements in the second and third row of the periodic table have electrons
in two or three orbits respectively
in orbits that can hold 8 electrons
in two orbits only
in two shells only
in two or three orbits holding 8 electrons each
Elements can be grouped into rows and columns in the periodic table because of the way ( ) fit into Bohr orbits of atoms.
electrons
protons
neutrons
shells
Each orbit or shell has a maximum number of electrons it can hold. This phenomenon is called:
the exclusion principle
the parking lot principle
the commons principle
All the elements in the first column of the periodic table have:
one electron in their outer Bohr orbit
one electron in their inner shell
eight electrons in their outer Bohr orbit
eight electrons in their outer shell
All the elements in the second column of the periodic table have:
two electrons in their outer Bohr orbit
two electrons in their inner shell
seven electrons in their outer Bohr orbit
seven electrons in their outer shell
The artificial elements with atomic numbers from 95 to 109 are characterized by:
unstable nuclei
breaking down quickly into groups of simpler atoms
light weight
non-radioactive
No new element has been discovered since 1982 in Darmstadt, Germany. It has an atomic number of:
109
94
103
120
130
Theorists think that when we get to atomic numbers in the region of 120 to 130:
a new group of stable elements will be found
a group of superheavy elements will be found
a new group of superreactive elements will be found
there will be no elements of such size
there can be no machine that can make such elements
