General Chemistry

Question 1

Does the electronegativity increase or decrease when you move up groups? Why?

Answer 1

increases because the smaller the atom, the more the nucleus is able to act on everything around it, it is not shielded by electrons

Question 2

Does electronegativity increase of decrease when going left in period? Why

Answer 2

Decreases. This is because, atom is farther from its goal. When it is closer, it becomes more electronegative

Question 3

Electronegativity

Answer 3

tendency of an atom to draw or polarize bonding electrons toward itself

Question 4

When you go left on the periodic table, what happens to the size of the atoms?

Answer 4

The size increases. Less effective charge because less valence electrons. Electrons don’t pull in as much

Question 5

When going up in groups, What happens to the size of the atom? Why?

Answer 5

Decreases. As you decrease the number of orbitals, you decrease the radius. As you go down the groups, the number of orbitals increases and so atom is bigger

Question 6

Ionization Energy

Answer 6

The energy to ionize—>energy required to remove an electron from an atom

Question 7

Electron Affinity

Answer 7

Energy that is released why electron is added

Question 8

What does it mean for an atom to have low ionization energy

Answer 8

electrons can be easily removed from those atoms

Question 9

What does it mean for an electron to have high affinity

Answer 9

means atoms will easily accept electrons

Question 10

Atoms with low ionization energy (left side of table) will bond with atoms that have____

Answer 10

high electron affinity. easily accepts electrons because the low ionization electron easily gives electron

Question 11

What are metalloids and where are they on the table

Answer 11

They are semimetallic elements and they are between metals and nonmetals

Question 12

Where are the nonmetals

Answer 12

Question 13

Where are metals

Answer 13

Question 14

periods on the periodic table represent atoms with:

Question 15

An element is a

Answer 15

pure chemical substance that consist of a single type of atom, distinguished by its atomic number

Question 16

Why do elements with larger shell sizes have low ionization energy? Where are they in terms of groups.

Answer 16

this is due to sheilding (by the inner shell electrons) from the positive charge of the nucleus. The greater the distance between the electrons and the nucleus, the less energy is needed to remove the outer valence electrons (because of less pull)

Question 17

The attraction of the nucleus on the outermost electron in an atom tends to : (Increase or decrease) from right to left and top to bottom

Answer 17

Decrease.The attraction of the nucleus on the outermost electrons determine the ionization energy, which increases towards the right and increases up on the periodic table