Understanding the Periodic Table

Question 1

Ionization energy

Answer 1

The amount of energy required to remove an electron from a gaseous atom

Question 2

Ionization group trend

Answer 2

It decreases as you go down a group because of more energy levels because if closer to nucleus it is harder to remove
Increases as you go across a period because each atom is trying to become a noble gas and is holding on more tightly to the electrons so harder the closer to noble gases you get

Question 3

Does it require more energy (in ionization energy) to remove a 2nd or 3rd electron?

Answer 3

Yes because they are more attracted to the nucleus

Always more energy needed - larger number - for more electrons

Question 4

Is there a very large increase of ionization energy whenever an electron is removed from an atom that is isoelectronic with a noble gas?

Answer 4

Yes, more attracted to staying with 8 electrons

IE goes up a lot

Question 5

Electronegativity

Answer 5

Tendency for an element to attract electrons with chemically combined with another element

Question 6

What element has the highest EN?

Answer 6

Fluorine

Question 7

Electronegativity group trend

Answer 7

Decreases as you go down a group because electrons are less attracted to the nucleus due to more energy levels
Increases across period because electrons are most attracted to the nucleus and becoming isoelectronic with a noble gas

Question 8

Cations rule (+)

Answer 8

Cations are always smaller than the neutral atom because there is a loss of electrons and more protons than electrons and electrons are pulled in closer to the nucleus

Question 9

The more electrons lost…

Answer 9

The smaller the atom becomes

Question 10

Anions rule (-)

Answer 10

Anions are always larger than the neutral atom because more electrons than protons results in less attractive force and the electrons are thus not pulled in closer to the nucleus

Question 11

The more electrons gained…

Answer 11

The bigger the ion becomes