Ionization Energy
Atomic Radius
Electronegativity
Electron Affinity
Groups
Valence electrons/ Ions
100

An Ion

what is an atom with a positive or negative charge

100

define atomic radius

what is half the distance between two adjacent nuclei of atoms of the same element. 

100

Define electronegativity

Electronegativity tells us how strongly an atom holds onto/attracts electrons to itself. 

100

Metals form _______ and nonmetals form _________

what are Cations and anions

100

Name of the group of elements that have 1 valence electron with the exception of hydrogen

What are Alkali metals

100

What charge will a lithium ion have

Li1+

200

Define ionization energy

What is the energy required to remove one valence electron. 

200

The direction the trend in atomic radius increases

what is Increases from top to bottom within a group, decreases from left to right within a period. 

200

The direction the trend in electronegativity increases

what is decreases from top to bottom within a group, and it increases from left to right within a period.  

200

This group gains electron the easiest, making them the group with the highest electron affinity

what are halogens

200

The name for elements with 2 valence electrons 

What are Alkaline Earth metals

200

What charge will an oxygen ion have

O2-

300

The directions the trend of Ionization energy is increasing

What is decreasing from top to bottom within a group, increases from left to right within a period. 

300

Name the largest element:

Mg, Al, Cl

Mg

300

Order the following elements in increasing electronegativity: 

N, F, C, Be 

Be, C, N, F

300

electron affinity _________ down a group because its valence electrons are further away

what is decreases

300

The name of the most stable group on the periodic table 

what are Noble Gases

300

This groups is the most reactive among the metals

what are alkali metals

400

If it's easy to remove an electron, is ionization energy low, or high?

what is Low

400

Review: What is the electron configuration of Ca

1s22s22p63s2

400

The most electronegative element on the periodic table

what is Florine 

400

Arrange the following elements in order of increasing electron affinity:

Al, S, Mg, Cl, F

Mg, Al, S, Cl, F 

400

These elements are extremely toxic and have 7 valence electrons.

what are Halogens.

400

What are two elements that don't follow the octet rule?

what are Hydrogen and helium

500

Explain why we observe the periodic trends in ionization energy.  

It decreases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nucleus. The attracting forces become weaker.  

It increases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons and makes them harder to remove, which increases ionization energy.

500

Explain why we observe the periodic trends in atomic radius.  

It increases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nucleus. 

It decreases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons which pulls them in and makes the atom smaller. 

500

Explain why we observe the periodic trends in electronegativity. 

It decreases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nucleus. The attraction becomes weaker so the atoms ability to attract electrons becomes weaker 

It increases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons, thus increasing electronegativity. 

500

Halogens release or gain energy by adding and electron?

what is release (exothermic)

500

Why are noble gases chemically stable?

They have an octet. 

500

Name the ion that is least likely to form:

Ca2+, Na+, Li2+

Li2+

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