Atom, Molecules, And Ions

Question 1

Group 1A

Answer 1

Alkaline Metals
(1+)
-highly basic
-React rapidly with water 
- never found in pure state in nature

Question 2

Group 2A

Answer 2

Alkaline earth meals
(2+)
-less reactive
-never found in nature in pure state

Question 3

Groups 3-12 (3B-2B)

Answer 3

Transition metals

Question 4

Group 17 (7A)

Answer 4

Halogens
(-1)
-colorful, corrosive nonmetals
-not found in pure state in nature

Question 5

Group 18 (8A)

Answer 5

Noble gasses

-colorless gasses with very low chemical reactivity

Question 6

Metals

Answer 6

• all except mercury are found at room temp.
• malleable
• good conductors

Question 7

Non-metals

Answer 7

• All on right side of zig-zag line, except Hydrogen
• when solid…
  - Brittle, poor conductors

Question 8

Metalloids

Answer 8

-properties are intermediate between those of metals and nonmetals

Question 9

Intensive property

Answer 9

Does not depend on amount

• density
• melting point

Question 10

Extensive property

Answer 10

Does depend on amount

• length
• volume

Question 11

Physical properties

Answer 11

Does not involve change in chemical makeup

Question 12

Chemical property

Answer 12

Does involve change in chemical makeup

Question 13

Atoms of different elements joined together in many different ways

Answer 13

Chemical compound

Question 14

Each chemical compound is described by its…

Answer 14

Chemical formula

Question 15

A chemical reaction is written via a…

Answer 15

Chemical equation

Question 16

Law of Mass conservation

Answer 16

Mass is neither created nor destroyed in chemical equations

Question 17

Law of definite proportions

Answer 17

Different samples of a pure chemical compound always contain the same proportion of elements by mass

Question 18

Law of multiple proportions

Answer 18

Elements can combine in different ways to form different chemical compounds whose mass ratios are simple, whole-number multiples of each other

Question 19

Cathode ray tubes/Thomson

Answer 19

Discovery of electrons

Question 20

Gold foil/Rutherford

Answer 20

Discovery of Protons and Neutrons

Question 21

Dalton’s theory of matter

Answer 21

• elements are made of tiny particles called atoms
• each element is characterized by the mass of its atom
• fractional parts of elements are never involved in chemical reactions
• Chemicals only rearrange, atoms themselves do not change

Question 22

Atomic Number

Answer 22

• Number of protons in nucleus

- number of electrons in neutral form

Question 23

Mass number

Answer 23

of protons + # of Neutrons

Question 24

Writing mass and atomic # together in the elemental symbol

Answer 24

Mass # = superscript

Atomic # = subscript

Question 25

Atomic weight

Answer 25

Weighted average of the elements naturally occurring isotopes

Question 26

Mole and Molar Mass

Answer 26

One mole of any element is the amount whose mass in grams (molar mass) is equal to its atomic weight

Question 27

Avogadro’s Number

Answer 27

6. 022141x10^23 | - equal to the amount of atoms in 1 mol of any element

Question 28

Covalent bond

Answer 28

- sharing electrons | - creates a molecule

Question 29

diatomic elements

Answer 29

- only exist in pairs of themselves - 7 to heaven - H, N, O, F, Cl, Br, I

Question 30

Binary Ionic compounds

Answer 30

- only 2 elements - gain or loss of electrons - involve cation (+) and anion (-) - naming... - positive ion first, name does not change - negative ion 2nd, ending of element changes to “-ide”

Question 31

Cations & Anions

Answer 31

- metals tend to form cations - nonmetals tend to form anions - find charge using location (group) on periodic table (1+) (2+) (3+) (3-) (2-) (1-)

Question 32

!!!!!

Answer 32

- using Roman numerals to create a neutral compound - all about charges, an number of each element - cross drop

Question 33

Polyatomic ions

Answer 33

-first cation, then anion -usually end in “-ite” or “-ate” Oxoanions- has different # of oxygen atoms

Question 34

Finding AMU using isotopes

Answer 34

(M1P1 + M2P2 +...) / # of isotopes ``` M= mass of isotope P= percent abundance of isotope (decimal) ```