Let’s Play Sit in teams of 4.

Periodic Table- History and Organization

Periodic Families

What is my size?

Giving up electrons

I love electrons!

Potpourri

Periodic Table- History and Organization Periodic Families What is my size? Giving up electrons I love electrons! Potpourri

$100 He is sometimes called the “father of the Periodic Table”

Mendeleev

$200 On the original periodic table, elements were organized by similar properties and this

Atomic mass (or weight)

$300 These are the two ways elements on the modern periodic table are organized

Similar properties and atomic number

$400 The name given to rows on the periodic table

Periods (rows)

$500 These elements tend to lose electrons and are found on the left side of the periodic table

Metals

$100 Lithium is a member of this family of highly reactive metals

Alkali metals

$200 Chlorine is a member of this family

Halogens

$300 Xenon is a member of this family

Noble Gases

$400 Atoms of elements in this family tend to lose two electrons

Alkaline Earth Metals

$500 Thorium is a member of this family

Actinide Family

$100 Which has a smaller atomic radius, cesium (Cs) or potassium (K)?

Potassium

$200 Which is bigger, a neutral atom or its cation?

The neutral atom is larger

$300 Which has a larger radius, a neutral atom or its anion?

The anion has a larger radius

$400 What is the general trend for atomic radii as you move from left to right across a row on the periodic table?

Atomic radius decreases; increasing nuclear charge pulls electrons is closer

$500 What is the reason for the difference in size between a neutral atom and its cation?

The cation has lost (electrons) an entire energy level

$100 What is the general trend in ionization energy as you move down a group on the periodic table?

Ionization energy decreases

$200 What is the general trend in ionization energy as you move across a period from left to right?

IE increases

$300 What is the difference between first, second, and third ionization energies?

1 st IE<2 nd IE<3 rd IE Or 1 st IE= energy to remove the first electron, 2 nd is to remove the second, etc.

$400 What is the name given to columns of the Periodic Table?

Groups

Daily Double!

Daily Double! Why does atomic radius decrease from left to right across a period?

The number of protons increases, thereby increasing the nuclear charge and the force of the nucleus on the electrons. The increased nuclear force pulls the electrons in closer

$100 The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called this.

Electronegativity

$200 Why does electronegativity increase as you move from left to right on the periodic table?

Effective nuclear charge increases and radius decreases, increasing the force/pull of the nucleus on electrons

$300 What is the name for the energy released when an electron is added to an atom?

Electron affinity

$400 What is the most electronegative element?

Fluorine

$500 This is when the layers of core electrons block the valence electrons from feeling the force of attraction of the nucleus.

Shielding effect

$100 These are the most reactive metals

Alkali metals

$200 The outer shell electrons involved in bonding are called this.

Valence electrons

$300 Metals tend to ___________ electrons to become ___________

Lose, cations

$400 Put the following atoms in order from lowest to highest ionization energy (first IE) Ba, Cu

Ba<Cu

$500 Put the following atoms in order from smallest to the largest atomic radii. Mg, P

P<Mg

FinalJeopardy

Periodicity

The shielding effect is one of the three primary factors that affect the periodic trends. Name or describe the other two.

1. Nuclear charge (number of protons in the nucleus) 2. Highest energy level (or number of energy levels)

Daily Double!