Periodic Table (Finals)
structural purposes
Transition metals are primarily used for
protons and neutrons can be subdivided into this by colliding them.
quarks
with more electrons than protons
A negative ion is an atom
chemically active
Because fluorine has one electron less than a stable number in its outer level, it is
noble gas
Because helium has an atomic number of 2, it is an example of
atomic period
Each horizontal row in the periodic table correspond to an
2
How many electrons are unpaired in the outermost shell of sulfur (S, atomic number 16)?
all of the above
If an election of atomic number 118 is ever synthesized, it would be 1. chemically inert 2. radioactive 3. a gas at room temperature 4. all of the above
a column on the right side
In the periodic chart, all noble gases are listed in
range from metals to nonmetals
In the periodic chart, the elements listed in rows between alkali metals and the noble gases
have different properties that are unlike those of other atomic groups
The inner transition metals are not listed in the main body of the periodic table because they
A capital letter or a combination of a capital letter and a small letter that is used to represent an element.
atomic symbol
an average of the masses of all the isotopes that occur in nature for an element.
average atomic mass
The region around the nucleus occupied by electrons.
electron cloud
the particles that move about the nucleus and have a negative charge.
electrons
vertical columns of elements
groups
Atoms of the same element but with different numbers of neutrons.
isotopes
A total count of the neutrons and protons in an atom.
mass number
Elements that have some properties of both metals and nonmetals charge.
metalloids
elements that are found on the left side of the periodic table.
metals
the center of an atom where protons and neutrons are located.
nucleus
A chart that shows the classification of elements.
periodic table
the horizontal rows of elements
periods
elements in the middle of the periodic table, periods 4 through 7.
transition elements
Strontium and calcium are in the same atomic group, hence they have similar physical and chemical properties.
A radioactive isotope of strontium, Sr, is especially dangerous to humans because it tends to accumulate in bone marrow tissues. How does this relate to the organization of the periodic table?
chemically active
Alkali metals and halogens are similar because both
there is no more room in its outermost occupied shell
Although the effective nuclear charge in the outer shell of a neon atom is relatively strong (about +8), neon has no affinity for an additional electron because
all its energy levels filled
An atom with a stable electron arrangement does not add or lose electrons easily since it has
adds more energy to the gas atoms
An electric current passing through gas
more mass means more protons, which act to pull electrons in closer to the nucleus.
As atoms get more massive, they become smaller in size because
nonmetals
At room temperature and atmospheric pressure, examples of elements in all three phases can be found within the
these electrons are able to pair with unpaired valence electrons; the nuclear charge attracts them; there are three more spaces available in their outermost shell.
Both nitrogen and phosphorus are able to attract three more electrons to their outer shells because
atomic group
Each vertical column in the periodic table corresponds to an
are members of the same chemical family
Each vertical column of the periodic chart lists elements that
transition metals
Elements in group 3 through 12 are
atomic number
Elements of the periodic table are listed in order of
do not have similar properties
Helium, He, and beryllium, Be, are both the second elements in their respective intervals. They are not placed directly above each other in the periodic table because they
periods
Horizontal rows of the periodic table are called
The more massive atoms have a greater number of atomic shells.
How is it possible that as atoms get more massive they become larger in size?
3
How many atomic shells are completely filled for the chlorine ion, Ch^1- (atomic number 17)?
6
How many atomic shells are occupied by electrons in the gold atom (atomic number 79)?
5
How many electrons are in the outermost shell of phosphorus (P, atomic number 15)?
2
How many electrons are in the outermost shell of strontium (Sr, atomic number 38)
3
How many electrons are unpaired in the outermost shell of aluminum (Al, atomic number 13)?
diagonally just right of the center
In the periodic table, the metalloids are found
the second electron experience a fare greater effective nuclear charge
It is relatively easy to pull an electron away from potassium atom, but very difficult to remove a second one because
using the properties
Mendeleev was able to predict the properties of a number of undiscovered elements
using the properties of neighboring elements in his periodic chart
Mendeleev was able to predict the properties of a number of undiscovered elements by
metals
Most of the elements in the periodic chart are
the charge of these ions corresponds to the number of valence electrons that may be lost.
The alkali metals tend to form +1 ion while the alkali earth metals tend to form 2+ ions because
equal to the electron capacity of the noble gas shells.
The number of electrons in a period is
it has one less shell containing electrons
The potassium ion, K1+, is smaller than the neutral potassium atom (K, atomic number 19) because
breaking when bent
The property that is not typical of a metal is 1. shiny appearance 2. breaking when bent 3. conduction of electricity 4. conduction of heat
false
The valence electrons of elements in the same atomic period are similar because elements in the same atomic period have the same number of paired valence electrons (True or False)?
a nonmetal
What type of solid would have the greatest tendency to shatter upon impact with a hammer?
move away from the nucleus
When added energy overcomes the attractive force between an electron and the nucleus of an atom, the electron would
releases the energy it has gained.
When an electron is pulled back toward the nucleus, it
Cl<Br<K>Rb
Which of the following shows elements in order of increasing atomic size (Cl, atomic number 15; K, atomic number 19; Br, atomic number 35; Rb atomic number 37)?
Bi<Tez<Br<Ar
Which of the following shows elements in order of increasing ionization energy (Ar, atomic number 18; Br, atomic number 52; Bi, atomic number 83)?
decreases gradually with periodic sudden drops
With increasing atomic number, the atomic size of elements
