Trends in the periodic table

Question 1

What are the 4 trends of the periodic table

Answer 1

1. Atomic radius
   2.Ionization energy
   3.Electron affinity
   4.Electronegativity

Question 2

What is atomic radius

Answer 2

the estimated size of the atom from the nucleus to the outer shell

Question 3

How does the atomic radius change over the periodic table

Answer 3

The radius gets bigger as you go down and to the left. Francium is big helium is small

Question 4

What is the shielding effect

Answer 4

The more layers of electrons there are, the less the outer electrons feel attraction to the nucleus. The outer electrons are also repelled by the inner electrons

Question 5

What happens to an atom as you go left to right on the periodic table? (period) why

in terms of atomic radius

Answer 5

The atomic radius decreases. While both protons and electrons are being added to the atom as we move right, the electrons are all on the same shell so it does not contribute to the shielding effect. This means the attractions force increases while the shielding effect stays mostly the same.

Question 6

What happens to an atom as you go top to bottom on the periodic table? (group)

Answer 6

The atomic radius increases. A lot of electrons are added. Electrons in the inner energy levels block or shield the valence electrons from the attraction of the nucleus. Electrons are not held as tightly

Question 7

What happens to a metal atom when it becomes an ion?

Answer 7

Metals lost electrons. There is less shielding effect. It gets smaller.

Question 8

What happens to a non metal atom when it becomes an ion

Answer 8

Non metals gain electrons . More electrons make more shielding effect. The electrons are less attracted to the nucleus. The atomic radius increases.

Question 9

What is ionization energy

Answer 9

The amount of energy required to remove an electron from a gaseous atom. The energy is measure in units of kJ/mol

Question 10

What is first ionization energy

Answer 10

The amount of energy needed to remove the first electron from the atom. The least attracted electron in the atom

Question 11

What are the trends of ionization energy along the periodic table

Answer 11

It increases as you go left to right on a period.
Decreases as you go down a group

Question 12

What are factors of ionization energy(3)

Answer 12

Nuclear charge - num of protons, strength of pull from nucleus
atomic radius - Distance between the nucleus and the outer electron
Shielding effect - how much are the inner electrons shielding the outer ones

Question 13

Trends of ionizatin energy

Answer 13

Increases left to right on a period
decreases down a group
opposite of atomic radius

Question 14

what is electron affinity

Answer 14

The energy change that happens when you add an electron to a stable gas atom, forming an anion.
Energy is often released
kj/mol

Question 15

Trend of electron affinity

Answer 15

increases from left to right and decreases down a group

The larger the amount of of energy released, the easier it is to add an electrons
due to increase in nuclear charge

Question 16

What does a very negative number of electron affinity mean.

Answer 16

indicates that a lot of energy is released when an electron is added to a gaseous atom, and that such a process is very likely to occur.

Question 17

what is electronegativity

Answer 17

The ability of an atom to attract the shared atoms in its bond
A high number means a high electronegativity and therefore a stronger attraction for electrons.

Question 18

How is electronegativity measured

Answer 18

It is a relative scale.
categorized using physical properties such as ionization energy
The highest is 4.0 for fluorine.

Question 19

What are the trends of electronegativity
and why

Answer 19

increases from left to right
- the number of protons increases but the shielding effect doesn’t. SO electrons are more attracted to the atom
Decreases down a group
- shield effect increases, electrons are less attracted to nucleus.