Review

Question 1

Define quantitative property

Answer 1

these are the measured properties involving #’s and units

Question 2

Define the term qualitative property

Answer 2

description or characteristics about substance using senses

Question 3

Describe where metals are

Answer 3

Left of the staircase

Question 4

Describe where non-metals are

Answer 4

Right of the staircase

Question 5

Describe where metalloids are

Answer 5

Stairs

Question 6

Describe physical change

Answer 6

changes that occur in shape,form,appearence or state. No new substance is formed

Question 7

Describe Chemical change

Answer 7

One or more new substances form in a reaction

Question 8

What are chemical change clues

Answer 8

C- colour changed
H-heat,light,sound
I-irreversible
P-percipitate ( soild, tiny flecks, thickening)
\+
G- gas formation (smoke, bubbles)
& order change

Question 9

What is matter divided into

Answer 9

Pure stubstance, and Mixtures

Question 10

What are pure substance divided into

Answer 10

Elements and Compounds

Question 11

What are mixtures divided into

Answer 11

Heterogenous, and Homogenous

Question 12

What is an observation

Answer 12

recording what happened durning a lab using your senses

Question 13

What is inferences

Answer 13

take observations and use prior knowledge to explain it

Question 14

Dalton

Answer 14

element exist as uncuttleable particle, thought charge less spheres

Question 15

Thomson

Answer 15

discovered the electron

cathode-ray tube experiment

Question 16

Rutherford

Answer 16

Nucleus’s, densely positive, electrons move, gold foil experiment, atom made of empty space

Question 17

Chadwick

Answer 17

Neutrons found in nucleus

Question 18

Bohr

Answer 18

Electrons orbit nucleus’s at set speed and energy level

Question 19

What is a Ion

Answer 19

a stable ion, an atom becomes stable by gaining or loosing electrons

Question 20

Caton

Answer 20

Have positive charges, these atom lost electrons and therefore metals

Question 21

Anion

Answer 21

Have negative charges, atom has gained electrons, non metals

Question 22

Isotopes

Answer 22

Atoms of an element that share the same number of electrons and proton but differ in mass. The neutrons

Question 23

Average atomic mass equation

Answer 23

Mass isotope x abundance + Mass isotope x abundance…

Question 24

What are the 4 types of Orbitals?

Answer 24

S orbitals
P orbitals
D orbitals
F orbitals

Question 25

S orbitals

Answer 25

Spherical shape, made of 1 su shell which can hold 2 electrons max

Question 26

P orbitals

Answer 26

Dumbbell in shape (3), made up of 3 su shells, hold up to 6 electron max

Question 27

D orbitals

Answer 27

Dumbbell In shape 5, made up of 5 subshells, can hold ten electrons max

Question 28

F orbitals

Answer 28

Dumbbell in shape (7), made up of 7 subshells and can hold up to 14 electrons max

Question 29

Electron configuration

Answer 29

Electrons get filled from lowest energy orbitals onwards. 1S is lowest orbital.

Question 30

Condensed Electron Configuration

Answer 30

Select last noble has that was passed through when deciding E.C looked like for the element Place symbol in bracket Then write only remaining E.C Fluorine [He] 2S2 2P5

Question 31

Energy Level Diagram Rules

Answer 31

Hund’s Rule— each subshells within an orbital must have 1 electron in each position Aufbaus rule- electrons must fill lower energy levels first

Question 32

Ionic Compounds Properties

Answer 32

- made up of 1 metal and 1 or more non metals - metals appear first - form crystal lattice structures-lots of bonds holding crystal together - soild at room temperature - soluble in water - form electrolytes - provide path for electrons to form on therefore are good conductors of heat and electricity (as a solution) - melting boiling point high due to the increased energy needed to break down crystal bonds

Question 33

Formation of Ionic Bonds

Answer 33

Gain or loose electrons to become stable

Question 34

3 step symbols

Answer 34

Draw Lewis Symbol for each element Show the ions ( gain and loose e) Show chemical formula

Question 35

What is an Ionic Bond

Answer 35

The electrostatic force of attraction between ion+ and ion-

Question 36

Formula unit

Answer 36

The smallest repeating unit in an ionic crystal

Question 37

Electrolyte

Answer 37

A compound that dissolves in water producing a solution that conducts electricity

Question 38

Ionic Compounds with Binary Metals

Answer 38

Metal found in group 1 and 2 + Al,Zn,Ag All have 1 ionic charge Metals appear first and name doesn’t change Non metal name changes to ide

Question 39

Ionic Compounds with Multivalent Metals

Answer 39

Metals found in group 3 all the way to the staircase 2 naming systems Stock Classical

Question 40

Stock Naming System

Answer 40

Involves using Roman numerals to represent the ionic charge for metals Always go with most common when haven’t been told Metal keeps name followed by Roman numerals Non metals change to ide

Question 41

Classical Naming System

Answer 41

Identifies ionic charge for metals using a suffix on the end of metals name Ic for the higher value Ous for lower All transition metals use this except the ones with one charge Metals change to ide

Question 42

Latin Root names

Answer 42

``` Iron:Ferrum Copper:Cuprum Tin:Stannum Lead:Plumbum Gold:Aurum ```

Question 43

Polyatomic Ions

Answer 43

are usually anion units meaning they have a common charge for 2 or more combined non metals Majority are called (oxyanions) because they have oxygen in the unit Metals keep name if binary or multivalent Non metal change to ate or ite if looses oxygen Exceptions apply

Question 44

6 Polyatomic Ions

Answer 44

``` Hydroxide - (OH)-1 Chlorate-(ClO3)-1 Nitrate-(NO3)-1 Sulfate-(SO4)-2 Carbonate(CO3)-2 Phosphate(PO4)-3 ```