Minerals Pt.1 (L4)

Question 1

5 main characteristcs to be truly considered a mineral?

Answer 1

1. is solid
2. is inorganic (non-living)
3. Definite chemical composition
4. naturally occuring
5. crystaline internal structure

Question 2

What’s a material that you wouldn’t think of as a mineral, but actually is?

Answer 2

Ice

Question 3

In which way are minerals and rocks different?

Answer 3

Rocks are typically made of minerals, but minerals don’t contain rocks

(minerals are the building blocks of rocks)

Question 4

What are minerals made of?

Answer 4

the atoms of one or more checmical elements

Question 5

What is an atom?

Answer 5

the smallest particle of matter that has the characteristics of an element.

Question 6

What is the nucleus of an atom made of?

Answer 6

Subatomic particles called Protons and Neutrons

Question 7

What are the cloud-like shells of a nucleus?

Answer 7

Electrons

Question 8

What is the mass and charge of a proton?

Answer 8

1 atomic mass unit, and a charge of +1

Question 9

What is the mass and charge of a neutron?

Answer 9

1 atomic mass unit, and no charge

Question 10

What is the mass and charge of an electron?

Answer 10

NO MASS, and a charge of -1

Question 11

Nearly all of an atom’s mass is in its nucleus? T or F

Answer 11

True

Question 12

2 categories of electrons

Answer 12

Valence electrons and Core electrons

Question 13

How is the Periodic Table organized (simplified)?

Answer 13

Toward the left = lose electrons

Toward the right = gain electrons

Question 14

What is the atomic number and where is it placed?

Answer 14

it denotes the number of protons in the atom

placed above the chemical symbol

Question 15

What is the atomic weight and where is it placed?

Answer 15

the full weight of one of the atom (atomic mass units)

under the chemical symbol

Question 16

How do you find the number of Neutrons through the atomic weight?

Answer 16

atomic weight - # of protons = # of neutrons

Question 17

what are the outermost electrons called?

Answer 17

Valence electrons

Question 18

What happens when an atom has less than 8 electrons in its outermost shell?

Answer 18

it bonds with other atoms

Question 19

Explain how ionic bonding occurs through mutual attraction of oppositely charged ions?

Answer 19

(A) atom with one valence electron gives it up to (B) atom who has 7 valence electrons

Now (B) electron has 8 and a full outermost shell and (A) now got rid of the useless one electron and its next shell in becomes its outermost electron shell (8 electrons)

Giving up electron = Positive charge 0- (-1) = +1
Accepting electron = Negative Charge 0-(+1) = -1

Now oppositely charged and oppsites attract so now IONICALLY BONDED

Question 20

How does a covalent bond happen?

Answer 20

involves the sharing of valence electrons

By sharing 2 electrons between the atoms, both atoms get their outermost shells filled and both are satisfied

Question 21

which is stronger, covalent bonds or ionic bonds? and why?

Answer 21

covalent bonds, b/c both atoms think they own the shared electrons and aren’t willing to give them up without a fight

Question 22

What contributes to the hardness of quartz?

Answer 22

the strong covalent bonds in quartz, within the silica units and also between the silica units

Question 23

What is an example of a very weak form of bonding? and why?

Answer 23

liquid water

oxygen is slightly negative and hydrogen slightly positive
so = weak bonds

“I like you, but not enough to stay with you for very long?

Question 24

What accounts for Graphite easily rubbing off on paper?

Answer 24

Graphite is made of internally strong sheets of carbon (Covalently bonded)

but these strong sheets are very weakly held together by very weak van der Waals forces

Question 25

Metallic Bonding

Answer 25

a special type of bonding that occurs in in pure metals
(copper, gold, and silver)

Question 26

How can we think of Metallic Bonding?

Answer 26

We can think ofelectrons involved in this being in an alternative lfiestyle

hopping from nucleus to nucleus (Free migration)
- this accounts for the strong ability of metals to CONDUCT electricity and its different shapes