Periodic Table Organization

Periodic Table

By Craig LaPerriere

Multiple Choice

What is a group

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

What is a period

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

What group is carbon in?

• 1

• 2

• 13

• 14

• 15

Multiple Choice

Where are the transition metals located

• Left side of table

• Top of table

• middle of table

• right side of table

Multiple Choice

Which is a transition metal?

• Aluminum

• Calcium

• Sodium

• Chromium

Multiple Choice

Which element is a Transition Metal

• Strontium

• Silicon

• Titanium

• Cessium

Multiple Choice

Which element is a Halogen?

• Argon

• Iodine

• Calcium

• Sodium

Multiple Choice

Why are halogens so reactive

• Need 7 valence electrons

• Need to lose 1 electron to be stable

• Need to add 1 electron to be stable

• They are super large atoms

Multiple Choice

Which element is a Noble Gas?

• Neon

• Chlorine

• Sodium

• Phosphorus

Multiple Choice

Why are noble gases not reactive

• Too few electrons

• Too many electrons

• They have a full set of electrons

• They need more electrons

Multiple Choice

Group 18

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Group 1

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Group 17

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

​Valence electrons:

​The electrons in an atom’s outermost orbitals; determine the chemical properties of an element.​

-Each group of representative elements (1,2, 13-18) have an assigned amount of valence electrons.

Multiple Choice

Noble Gases have how many valence electrons

• 1

• 2

• 6

• 8

Multiple Choice

Alkali Metals have how many valence electrons

• 1

• 2

• 6

• 8

​Why do elements form ions of a certain charge?

​Everybody wants the electron configuration of a noble gas! Its the lowest energy state :)

Multiple Choice

When Halogens form ions, what is the charge of the ion?

• 7 +

• 7 -

• 1 -

• 1 +

Multiple Choice

What charge of ion will Sodium form?

• 1-

• 1+

• 7-

• 2-

Multiple Choice

When Magnesium forms an ion, what charge will that ion have?

• +1

• +2

• -2

• -1

Multiple Choice

What charge of ion will Aluminum form?

• 1-

• 2+

• 3-

• 3+

Metals, Metalloids, and Nonmetals

• The periodic table is divided into 3 types of chemicals

• They are in alphabetical order: 1. Metal, 2. Metalloid, 3. Nonmetal

• Metals are the largest group

• Metalloids are the smallest group between metals and nonmetals.

Multiple Choice

Metals are on the:

• Left side

• Right Side

• Stairstep

Multiple Choice

Nonmetals are on the:

• Left side

• Right Side

• Stairstep

Multiple Choice

A student is studying a mystery substance. It breaks easily. It has a very dull luster. It doesn't conduct any electricity. What is the most likely substance this is?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

The same student works with a new substance. He concludes it conducts electricity very well. It has a very shiny luster. When he hammers it, it simply dents and flattens. What is the most likely substance type?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

The third substance the student works with is a little brittle. It is just a little shiny. When he tries to conduct electricity through it at first, it doesn't conduct, but upon heating up, it does start to allow electrons to flow. What is the most likely substance type?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

Order the following elements in terms of increasing electronegativity

F, At, I, Cl,

• F, Cl At, I

• At, F, Cl, I

• At, I Cl, F

• F, Cl, I , At

Multiple Choice

Which accurately describes nonmetals?

• Both malleable and ductile
• Often used in computer parts
• Poor conductors of electricity
• Always solid at room temperature

Multiple Choice

Which group on the periodic table is the most reactive Metals?

• Alkaline-earth metals - Group 2
• Alkali metals - Group 1
• Transition metals - Group 3-7
• Halogens - Group 17

Multiple Choice

Which group of elements is inert?

• Alkaline metals - Group 1
• Alkaline-earth metals - Group 2
• Transition metals Groups 3-8
• Noble Gases - Group 18

Multiple Choice

Which group includes some of the most familiar elements like nickel, iron, and copper?

• Inner transition metals
• Transition metals
• Halogens
• Noble gases

Multiple Choice

Which pair of elements would have similar properties due to the position in the periodic table?

• Calcium (Ca), Helium (He)
• Copper (Cu), Gold (Au)
• Lithium (Li), Beryllium (Be)
• Aluminum (Al), Zinc (Zn)

Periodic Trends

Review

Increasing Atomic Radius

Increasing Atomic Radius

Cation Radius < Neutral < Anion Radius

Increasing Ionization Energy

Increasing Ionization Energy

Decreasing Electronegativity

Increasing Electronegativity

Electronegativity

• Increases as you move across the periodic table.

• Group 1 and 2 metals are the least electronegative elements and tend to lose electrons when forming ions.

• Nitrogen, oxygen, and halogens are the most electronegative and strongly attract electrons when in compounds.

• Decreases or stays the same moving down a group.

Multiple Choice

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

• decreases, increases

• increases, decreases

Multiple Choice

Which element has a higer Elecronegativity?

• Sulfur

• Oxygen

• Nitrogen

• Francium

Multiple Choice

Most elements on the periodic table are classified as __________.

• Metals
• Non-Metals
• Metaloids
• Gases

Multiple Choice

Order the following elements in terms of increasing atomic radii

Ca, Sr, Be , Mg

• Ca, Mg, Be, Sr

• Be, Mg, Ca, Sr

• Sr, Ca, Mg, Be

• Mg, Ca, Sr, Be

Multiple Choice

Order the following elements in terms of increasing electronegativity

Al, Mg, P, Cl

• Mg, Al, Cl, P

• Cl, P, Mg, Al

• Cl, P, Al, Mg

• Mg, Al, P, Cl

Ionization Energy

• The energy required to remove one electron from the outer shell of a neutral atom.

• This is the energy needed to form an ion.

• When ionization energy is high it is harder to remove that electron.

Multiple Choice

What is ionization energy?

• The energy required to remove an electron from a neutral atom

• The energy required to add an electron to a neutral atom

• The energy required to break a chemical bond

• The energy required to form a chemical bond

Multiple Choice

Order the following element in terms of increasing Atomic Radii

Si, Na, S, Mg

• S, Si, Mg, Na

• Na, Mg, Si, S

• S, Si, Mg, Na

• Na, Mg, S , Si

Multiple Choice

Which has the greater Electronegativity: 
N or C?

• C
• N