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