Unit 3, Periodic Table and Elements

Question 1

What is the center of an atom?

Answer 1

Nucleus

Question 2

What is outside the nucleus?

Answer 2

energy layers

Question 3

Where are electrons found in the atom?

Answer 3

The energy layers

Question 3

What is a cation?

Answer 3

It is a positively charged atom

Question 3

Where are protons and neutrons found in the atom?

Answer 3

The nucleus

Question 4

What is an anion?

Answer 4

A negatively charged atom

Question 5

What determines the identity of an element?

Answer 5

of protons

Question 6

What determines the weight of an element?

Answer 6

Protons and neutrons

Question 7

How much do protons and neutrons weigh?

Answer 7

1amu each

Question 8

How many electrons fit on the 1st energy level?

Answer 8

2 electrons

Question 8

What equation is for the # of electrons on each energy level?

Answer 8

2nsquared

Question 9

How many electrons fit on the 2nd energy level?

Answer 9

8 electrons

Question 10

How many electrons fit on the 3rd energy level?

Answer 10

18 electrons

Question 11

What is the most stable # of valence electrons?

Answer 11

8 valence electrons

Question 12

What did Mendeleev do?

Answer 12

He…
- arranged elements in increasing atomic mass
- stacked them by similar properties
- predicted properties of un-found elements

Question 13

What are the 3 types of elements?

Answer 13

• Metals
• Non-metals
• Metalloids

Question 14

What are properties of non-metals?

Answer 14

They…
- are bad conductors
- dull
- brittle
- gain electrons when reacting

Question 14

What are properties of metals?

Answer 14

They…
- are good conductors
- shiny
- malleable
- ductile
- lose electrons when reacting

Question 15

What are properties of Metalloids?

Answer 15

They are in between metals and non-metals

Question 16

What are Alkali metals?

Answer 16

They…
- are all metals, except for hydrogen
- have 1 valence electron
- very reactive
- Want to lose 1 valence electron

Question 17

What are Alkaline Earth metals?

Answer 17

They…
- metals
- have 2 valence electrons
- reactive, not as much as alkali metals
- want to lose 2 valence electrons

Question 18

What is the Boron Family?

Answer 18

They…
- metalloids + metals
- named after Boron
- 3 valence electrons
- want to lose 3 valence electrons

Question 19

What is the Carbon Family?

Answer 19

They…
- metals + non-metals + metalloids
- have 4 valence electrons
- many variations of bonds
- Want to lose or gain 4 valence electrons
- All organic molecules have carbon

Question 20

What is the Oxygen family?

Answer 20

They…
- metals + non-metals + metalloids
- have 6 valence electrons
- Want to gain 2 valence electron

Question 20

What is the Nitrogen Family?

Answer 20

They…
- metals + non-metals + metalloids
- have 5 valence electrons
- Want to gain 3 valence electrons

Question 21

What are Halogens?

Answer 21

They…
- are all non-metals
- have 7 valence electrons
- most reactive non-metals
- Want to gain 1 valence electron

Question 22

What are the Noble Gasses?

Answer 22

They…
- are all non-metals
- have 8 valence electrons
- don’t react, very stable

Question 23

Why are high atomic # atoms unstable?

Answer 23

They are unstable because they need a lot of protons - needs more neutrons - weakens attractive force on electrons - exist for very little time

Question 24

Why does the bottom left atoms of the periodic table have a bigger atomic radius?

Answer 24

This is because as we move to the rights of the periodic table there are more protons - more pull on electrons shrinking the atomic radius. Also, the bottom has more energy layers.

Question 25

Why are the bottom left and top right of the periodic table the most reactive?

Answer 25

The bottom left is reactive because they are metals that lose electrons when reacting so a lot more energy layers result in a weaker attractive force from the nucleus which makes it much easier for the electrons to transfer to a different atom. The top right is more reactive aside from the noble gasses because they have fewer energy layers resulting in a more attractive force pulling on the valence electrons which combined with the fact that non-metals gain electrons when reacting, makes it much easier for them to pull electrons from metals.