Periodic Trends

The Periodic Table:

Periodic Trends

• Trends are patterns seen in the periodic table.
• Trends are seen in mass, size, and reactivity.

Trends

​Lets Review the Parts of The Periodic Table

​You can do it!

Multiple Choice

The vertical (up and down) columns in the Periodic Table are called

• groups

• towers

• periods

• atomic numbers

Multiple Choice

The Modern Periodic Table of Elements is arranged by

• atomic mass
• atomic number
• valence electrons
• number of isotopes

Multiple Choice

What group is element A in?

• Alkali Metals

• Alkali Earth Metals

• Transition Metals

• Halogens

Multiple Choice

What group is element B in?

• Alkali Metals

• Alkali Earth Metals

• Transition Metals

• Halogens

Multiple Choice

What group is element C in?

• Alkali Metals

• Alkali Earth Metals

• Transition Metals

• Halogens

Multiple Choice

What group is element D in?

• Alkali Metals

• Alkali Earth Metals

• Transition Metals

• Halogens

Multiple Choice

What group is element E in?

• Halogens

• Alkali Earth Metals

• Transition Metals

• Noble Gases

Multiple Choice

Most of the periodic table is mode of _______.

• Metals

• Non-metals

• Semi-metals

Multiple Choice

The atoms along the staircase are called 

• metals
• nonmetals
• metalloids
• noble gases

Atomic Mass

The atomic mass of elements increases moving
down each group and right across each period.

Increasing Atomic Mass

We know that mass increases as the atomic number increases.....

Because there are more protons, it gets heavier.​

​Has nothing to do with the size.

​Atomic mass depends on Protons and Neutrons.

• The atomic radius is the distance from

the valence electrons to the nucleus.

• Simply put, it describes the size of an atom.

Atomic Radius

Increasing Atomic Radius

Lithium

Sodium

Potassium

Atomic Radius

The atomic radius of elements increases moving
down each group and left across each period.

Increasing Atomic Radius

Multiple Choice

As you move down a group, atomic radius increases because - 

• you add more and more neutrons
• you add more and more protons
• you add more and more shells (energy levels)
• you add more atomic mass

Multiple Choice

Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Multiple Choice

Of the halogens, which has the smallest radius?

• F

• Br

• He

• At

Multiple Choice

Which periodic group has the smallest atomic radius?

• Alkali metals
• Halogens
• Noble Gases
• Transition metals

Multiple Choice

What property is being measured in this diagram?

• Density

• Ionization Energy

• Atomic Radius

• Atomic Mass

Multiple Choice

Which of these elements in group 1A has the largest atomic radius?

• cesium

• rubidium

• potassium

• sodium

Multiple Choice

The atom with the largest atomic radius in Group 18 is - 

• Ar
• He
• Kr
• Rn

• Ionization energy is the energy required to

remove an electron from an atom.

• The more tightly electrons are held by the

nucleus, the harder they are to remove.

Ionization Energy

Energy Needed

to Remove Electron

-

-

+

+

​The smaller the size of the atom the more

Ionization Energy

The ionization energy of elements increases
moving up each group and right across a period.

Increasing Ionization Energy

​Opposite of atomic radius

Multiple Choice

Francium (Fr) has the lowest ionization energy in Group 1 because - 

• it has the smallest number of valence electrons
• it has the greatest atomic mass
• it has the greatest number of protons, so it attracts its electrons the strongest
• its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

Multiple Choice

Which group of elements has the lowest ionization energies?

• Alkali Metals (Group 1)

• Alkaline Earth Metals (Group 2)

• Halogens (Group 17)

• Noble Gases (Group 18)

Multiple Choice

What is the amount of energy required to remove an electron from an atom?

• atomic energy

• ionization energy

• ionic energy

• electron energy

Multiple Choice

As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more mass.
• the atoms have less mass
• the atoms have more protons.
• the atoms have less electrons.

Multiple Choice

As you move down the periodic table atoms get bigger.  This is because ____________.

• The atoms have more mass.
• The atoms have more protons.
• The atoms have more energy levels
• The atoms have more nuetrons

Multiple Choice

When across a period, the atomic size decreases so the first IE ___________.

• increases

• decreases

• constant

• i am not sure

• Electronegativity is a measure of how

strongly an atom is attracted to electrons.

• In bonds, electrons will be more attracted to

the atom with greater electronegativity.

Electronegativity

Attraction of electrons

to the nucleus
-

-

+

+

Electronegativity

The electronegativity of elements increases
moving up each group and right across a period.

Increasing Electronegativity

​Same as

Ionization Energy

Multiple Choice

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)

• Neon (Ne)

• Antimony (Sb)

• Germanium (Ge)

Multiple Choice

Which of the following halogens has the greatest electronegativity?

• Chlorine (Cl)

• Bromine (Br)

• Iodine (I)

• Astatine (At)

Multiple Choice

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

• ionization energy

• electropositivity

• electronegativity

• electron energy

Multiple Choice

Which element in period 4 has the highest electronegativity?

• potassium

• calcium

• copper

• bromine

Multiple Choice

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

• ionization energy

• electropositivity

• electronegativity

• electron energy

• Reactivity is the tendency of an atom or

molecule to undergo a chemical reaction.

• Certain elements react very easily with just

water. Other elements do not react at all.

• Note: Noble Gas elements (Group 18)

are not reactive. They are excluded.

Reactivity

Reactivity of Metals

The reactivity of metals increases moving
down each group and left across each period. Because it gets easier to remove electrons

Increasing Reactivity of Metals

​Same as

atomic radius

Reactivity of Non-Metals

Increasing Reactivity of Non-Metals

The reactivity of non-metals increases moving
up each group and right across each period.

Because it is easier to gain electrons.

​

Reactivity of Non-Metals

• Fluorine is the most reactive non-metal.

• Francium is the most reactive metal.

F

Fr

9
F

Fluorine

18.99

87
Fr
Francium

223

Multiple Choice

What metal is most reactive

• lithium

• sodium

• potassium

• rubidium

Multiple Choice

What non-metal is the most reactive

• iodine

• sulfur

• oxygen

• fluorine