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History and Periodic Law
Categories of Elements
Periodic Trends
Period Trends
100

There are 7 periods in the period table equal to the number of _________ 

Energy Levels

100

What are the three major categories of elements?

Metals, Nonmetals, and Metalloids

100

The Atomic Radius is _______ the distance between two adjacent atoms. 

Half

100
What is the ability of an atom to attract or gain electrons called? 

Electronegativity

200

The number of ______ determines the reactivity of elements

Valence Electrons

200

What is Group 1 of the period table called?

Alkali Metals

200

What is it called when inner shell electrons block the attraction between the nucleus and valence electrons.  

Electron Shielding 

200

What is ionization energy?

Energy required to remove an electron from the electron cloud

300

What is the repeating pattern in which the properties repeated every eighth element called? 

Law of Octaves

300

Transition Metals form ________ in solutions. 

Colored Ions

300

As you go down a group and the energy levels increase, the ______ between the nucleus and valence electrons increases and thus ______ the attraction. 

1. Distance

2. Weakens/Decreases

300

As you go across a period and the number of protons increase, the _______ increases and thus _______ the attraction. 

1. Nuclear Charge

2. Strengthens/Increases

400

What do you call when you have only two electrons to complete an energy level?

A Stable Duet

400

Metalloids have _____ (like metals) but are also ______ (like nonmetals)

1. Luster

2. Brittle

400

Why is electron shielding only a factor in group trends and not in period trends? 

All the elements in the same period have the same amount of energy levels

400

Electronegativity ______ as you go across a period and ______ as you go down a group. 

1. Increases

2. Decreases

500

Ekasilicon, Mendeleev's element, was discovered to be what actual element based on predicted properties? 

Germanium

500

What metal is not solid at STP?

Mercury (Hg)

500

Rank the atomic radius, ionization energy, and electronegativity between Fluorine (F) and Potassium (K). 

1. Atomic Radius: K > F

2. Ionization Energy: F > K 

3. Electronegativity: F > K

500

How are ionization energy and atomic radius correlated (directly or inversely) and why? 

Inversely

Ionization energy increases across a period and decreases as you go down a group while 

Atomic radius decreases across a period and increases as you go down a group