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chemistry > Review > Flashcards

Review Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

Define quantitative property

A

these are the measured properties involving #’s and units

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2
Q

Define the term qualitative property

A

description or characteristics about substance using senses

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3
Q

Describe where metals are

A

Left of the staircase

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4
Q

Describe where non-metals are

A

Right of the staircase

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5
Q

Describe where metalloids are

A

Stairs

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6
Q

Describe physical change

A

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

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7
Q

Describe Chemical change

A

One or more new substances form in a reaction

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8
Q

What are chemical change clues

A 
C- colour changed
H-heat,light,sound
I-irreversible
P-percipitate ( soild, tiny flecks, thickening)
\+
G- gas formation (smoke, bubbles)
& order change
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9
Q

What is matter divided into

A

Pure stubstance, and Mixtures

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10
Q

What are pure substance divided into

A

Elements and Compounds

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11
Q

What are mixtures divided into

A

Heterogenous, and Homogenous

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12
Q

What is an observation

A

recording what happened durning a lab using your senses

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13
Q

What is inferences

A

take observations and use prior knowledge to explain it

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14
Q

Dalton

A

element exist as uncuttleable particle, thought charge less spheres

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15
Q

Thomson

A

discovered the electron

cathode-ray tube experiment

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16
Q

Rutherford

A

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

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17
Q

Chadwick

A

Neutrons found in nucleus

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18
Q

Bohr

A

Electrons orbit nucleus’s at set speed and energy level

19
Q

What is a Ion

A

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

20
Q

Caton

A

Have positive charges, these atom lost electrons and therefore metals

21
Q

Anion

A

Have negative charges, atom has gained electrons, non metals

22
Q

Isotopes

A

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

23
Q

Average atomic mass equation

A

Mass isotope x abundance + Mass isotope x abundance…

24
Q

What are the 4 types of Orbitals?

A

S orbitals
P orbitals
D orbitals
F orbitals

25
Q

S orbitals

A

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

26
Q

P orbitals

A

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

27
Q

D orbitals

A

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

28
Q

F orbitals

A

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

29
Q

Electron configuration

A

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

30
Q

Condensed Electron Configuration

A

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

31
Q

Energy Level Diagram Rules

A

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

32
Q

Ionic Compounds Properties

A
  • 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
33
Q

Formation of Ionic Bonds

A

Gain or loose electrons to become stable

34
Q

3 step symbols

A

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

35
Q

What is an Ionic Bond

A

The electrostatic force of attraction between ion+ and ion-

36
Q

Formula unit

A

The smallest repeating unit in an ionic crystal

37
Q

Electrolyte

A

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

38
Q

Ionic Compounds with Binary Metals

A

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

39
Q

Ionic Compounds with Multivalent Metals

A

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

40
Q

Stock Naming System

A

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

41
Q

Classical Naming System

A

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

42
Q

Latin Root names

A 
Iron:Ferrum
Copper:Cuprum
Tin:Stannum
Lead:Plumbum
Gold:Aurum
43
Q

Polyatomic Ions

A

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

44
Q

6 Polyatomic Ions

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

chemistry (7 decks)

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