Ch 2 - Elements + The Periodic Table
Ch 2 - Elements + The Periodic Table
Chemical SymbolsChemical SymbolsAlways start with:Can be ___ or _____ letters
Always start with:Can be ___ or _____ letters
Periodic Table:color code your table!
Periodic Table:color code your table!
Metals, Non-metals, Metalloids
Metals, Non-metals, Metalloids
Fill in the graphic organizer to record the basic properties of groupings on the periodic table!
Fill in the graphic organizer to record the basic properties of groupings on the periodic table!
Metals Metalloids Non-metalsProperties: Properties: Properties:
STP state: STP state: STP state:
Appearance:
Conductivity:
Malleability:
Ductility:
Appearance:
Conductivity:
Malleability:
Ductility:
Appearance:
Malleability:
Conductivity:
Ductility:
Alkali metals: a.k.a. Group 1 Halogens: a.k.a. Group 17
Elements:
Key features:
Elements:
Key features:
Common uses:
Other:
Common uses:
Common uses:
Other:
Alkaline earth metals: a.k.a. Group 2 Noble gases: a.k.a. Group 18
Other:
Elements:
Key features:
Common uses:
Other:
Elements:
Key features:
READING the
TABLE
READING the
TABLEAtomic # Tells us:Atomic MassTells us: Therefore, The # of neutrons =
Atomic # Tells us:Atomic MassTells us: Therefore, The # of neutrons =
Practice: Practice:
NEUTRAL Atoms of the Elements! Name Symbol Atomic
# Atomic Mass
# of protons
# of electrons
# of neutrons
Bromine Mn 79 13 82
NEUTRAL Atoms of the Elements! Name Symbol Atomic
# Atomic Mass
# of protons
# of electrons
# of neutrons
Bromine Br 35 80 amu 35 35 45 Manganese Mn 25 55amu 25 25 30 Gold Au 79 197 79 79 118 Aluminum Al 13 27 13 13 14 Lead Pb 82 207 82 82 125
Do the Atomic Structure Worksheet
Do the Atomic Structure Worksheet
Name of Element
Symbol of Element
Atomic Number
Atomic Mass
Number of Protons
Number of Electrons
Number of Neutrons
K
35
Al
Li
12
8
Ni
10
18
Gold
11
Pb
Name of Element Symbol Atomic Number
Atomic Mass
Number of Protons
Number of Electron
Number of Neutrons
Potassium K 19 39 19 19 20
Bromine Br 35 80 35 35 45
Aluminum Al 13 27 13 13 14
Lithium Li 3 7 3 3 4
Magnesium
Mg 12 24 12 12 12
Oxygen O 8 16 8 8 8
Nickel Ni 28 59 28 28 31
Neon Ne 10 20 10 10 10
Argon Ar 18 40 18 18 22
Gold Au 79 197 79 79 118
Sodium Na 11 23 11 11 12
Lead Pb 82 207 82 82 125
Chemical FormulasChemical Formulas
tell you which elements are present in a compound, and their amount
Each new element is denoted by a CAPITAL LETTER.
NaCl = sodium and chlorineMgBr =magnesium and bromine
tell you which elements are present in a compound, and their amount
Each new element is denoted by a CAPITAL LETTER.
NaCl = sodium and chlorineMgBr =magnesium and bromine
The subscript (the small number slightly below the line) tells you how many atoms are present – that number only applies to the element at the immediate left of the number.
The subscript (the small number slightly below the line) tells you how many atoms are present – that number only applies to the element at the immediate left of the number.
Ex. H2O = 2 hydrogen atoms
1 oxygen atom
CaCl2 = 1 calcium atom
2 chlorine atoms
Ex. H2O = 2 hydrogen atoms
1 oxygen atom
CaCl2 = 1 calcium atom
2 chlorine atoms
Coefficients are large numbers written in front of the compound symbol. This tells you how many molecules of that compound you have.
Coefficients are large numbers written in front of the compound symbol. This tells you how many molecules of that compound you have.
Ex. 5NaNO3 = 5 Na atoms
5 N atoms15 O atoms
4NH4ClO3 = 4 N
16H4 Cl12 O
Ex. 5NaNO3 = 5 Na atoms
5 N atoms15 O atoms
4NH4ClO3 = 4 N
16H4 Cl12 O
Brackets around a complex ion, with a number to the immediate right of the brackets, tells you how many of that complex ions you have in the compound. That number applies to all elements inside the bracket.
Brackets around a complex ion, with a number to the immediate right of the brackets, tells you how many of that complex ions you have in the compound. That number applies to all elements inside the bracket.
Ex. (NH4)2SO4 = 2N, 8H, 1S, 4O
Ex. 4Ca3(PO4)2 = 4[3Ca 2P, 8O)]
= 12 Ca, 8P, 32O
Ex. (NH4)2SO4 = 2N, 8H, 1S, 4O
Ex. 4Ca3(PO4)2 = 4[3Ca 2P, 8O)]
= 12 Ca, 8P, 32O
Mg(NO3)2 =
3Ba3(PO4)2 =
Mg(NO3)2 =
3Ba3(PO4)2 =
1 magnesium atom2 nitrogen atoms6 oxygen atoms
9 Barium atoms6 potassium atoms24 oxygen atoms
Do the Reading Chemical Formula Worksheet
Do the Reading Chemical Formula Worksheet
Chemical Formula
Number of Different Types of Atoms
Names of Each atom present
Number of each type of atom
Total Number of Atoms present
Number of molecules of this compound
Ex. 2NaCl 2 SodiumChlorine
2 sodium2chlorine
4 2
3N2O3
2KHCO3
5FeSO3
C6H12O6
3K2Cr2O7
CH3COOH
Mg(OH)2
3 Al(OH)3
4CuClO3
Chemical Formula Number of Different Types of Atoms
Names of Each atom present
Number of each type of atom
Total Number of Atoms present
Number of molecules of this compound
Ex. 2NaCl 2 SodiumChlorine
2 sodium2chlorine
4 2
3N2O3
2 NitrogenOxygen
6 N9O
15 3
2KHCO3
4 Potassium HydrogenCarbonOxygen
2 Potassium2 Hydrogen2 Carbon6 Oxygen
12 2
5FeSO3
3 IronSulphurOxygen
5 Iron5 Sulphur15 Oxygen
25 5
C6H12O6
3 CarbonHydrogenOxygen
6 Carbon12 Hydrogen 6 Oxide
24 1
Chemical Formula Number of Different Types of Atoms
Names of Each atom present Number of each type of atom
Total Number of Atoms present
Number of molecules of this compound
3K2Cr2O7
3 PotassiumChromiumOxygen
6 Potassium6 Chromium21 Oxygen
33 3
CH3COOH3 Carbon
HydrogenOxygen
2 Carbon4 Hydrogen2 Oxygen
8 1
Mg(OH)2
3 MagnesiumOxygenHydrogen
1 Magnesium2 Hydrogen2 Oxygen
5 1
3 Al(OH)3
3 Aluminum OxygenHydrogen
3 Aluminum9 Oxygen9 Hydrogen
21 3
4CuClO3
3 CopperChlorideOxygen
4 Copper4 Chloride12 Oxygen
20 4
Study for Quiz!Study for Quiz!
Atomic Structure worksheetReading Chemical Formula
WorksheetModels of Molecules
Atomic Structure worksheetReading Chemical Formula
WorksheetModels of Molecules
Drawing Bohr Diagrams of
Atoms
Drawing Bohr Diagrams of
Atoms
The nucleus contains all the protons and neutrons.
Consequently, all the mass is concentrated in the nucleus. The electrons are arranged in specific ORBITALS around the nucleus.
The nucleus contains all the protons and neutrons.
Consequently, all the mass is concentrated in the nucleus. The electrons are arranged in specific ORBITALS around the nucleus.
Orbital LimitsOrbital Limits
There is a specific limit to how many electrons an orbital (or shell) can hold.
Within the orbitals, the electrons like to spread themselves out.
There is a specific limit to how many electrons an orbital (or shell) can hold.
Within the orbitals, the electrons like to spread themselves out.
Why Spread out?Why Spread out?
electrons carry negative charges negative charges repel
electrons carry negative charges negative charges repel
Electrons fill the orbitals in the following pattern:
Orbital: 1st 2nd 3rd 4th
2e- 8e- 8e- 18e-
Electrons fill the orbitals in the following pattern:
Orbital: 1st 2nd 3rd 4th
2e- 8e- 8e- 18e-
Which of these diagrams is incorrect? What elements are A,B,C,and D
Once an orbital is full, the electrons will start filling the next orbital.
The innermost orbital (#1) gets filled first.
Once an orbital is full, the electrons will start filling the next orbital.
The innermost orbital (#1) gets filled first.
Example: HydrogenExample: Hydrogen
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
1
1
1
0
1
Example LithiumExample Lithium
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
3
7
3
4
3
Example: ChlorineExample: Chlorine
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
Now do the worksheet:
“Models of the elements”
Atomic # = ______Atomic Mass = ______ # protons = ______# neutrons = ______ # electrons = ______
Now do the worksheet:
“Models of the elements”
17
36
17
19
17
The Valence Shell
The Valence Shell
Definitions: 1) Valence
Shell: the outermost orbital (or shell)
2) Valence Electrons: _electrons in the outside shell
Definitions: 1) Valence
Shell: the outermost orbital (or shell)
2) Valence Electrons: _electrons in the outside shell
The Valence Electrons are involved in forming bonds with other atoms. The inner electrons and nucleus are not involved in bonding.
The Valence Electrons are involved in forming bonds with other atoms. The inner electrons and nucleus are not involved in bonding.
Atoms can: - _gain valence electrons - _lose valence electrons - _share valence electrons
Atoms can: - _gain valence electrons - _lose valence electrons - _share valence electrons
Example: Oxygen Atomic # = _8____ Mass = ___16___ #p = _8___ #e = _8___ #n = _8___
Example: Oxygen Atomic # = _8____ Mass = ___16___ #p = _8___ #e = _8___ #n = _8___
Combining Capacity: The number of electrons that an atom must gain or lose to have a full valence shell.
Full for 1st shell = _2e-___Full for 2nd shell = _8e-___Full for 3rd shell = _8e-___
Combining Capacity: The number of electrons that an atom must gain or lose to have a full valence shell.
Full for 1st shell = _2e-___Full for 2nd shell = _8e-___Full for 3rd shell = _8e-___
Will an Atom Gain or Lose Electrons?Valence electrons Gain/Lose?
greater than 4 gain less than 4 loseequal to 4 gain or lose
Will an Atom Gain or Lose Electrons?Valence electrons Gain/Lose?
greater than 4 gain less than 4 loseequal to 4 gain or lose
exception: HYDROGENThis element is unique because it has
the ability to either gain or lose one electron to “fill” its orbitals.
exception: HYDROGENThis element is unique because it has
the ability to either gain or lose one electron to “fill” its orbitals.
Examples: Nitrogen atomic # = _____ mass = _____ #p = _7____ #n = _7____ #e = _7____ # valence e = _5____ Will this atom gain or lose? __gain_ How many ? ___3____ What is its combining capacity? _3-_ Charge ? __3-
Examples: Nitrogen atomic # = _____ mass = _____ #p = _7____ #n = _7____ #e = _7____ # valence e = _5____ Will this atom gain or lose? __gain_ How many ? ___3____ What is its combining capacity? _3-_ Charge ? __3-
7
14
When nitrogen is charged it is called _nitride
When nitrogen is charged it is called _nitride
Example 2: Neon atomic # = _10____ mass = ___20__ #p = __10___ #n = __10___ #e = __10___ # valence e = __8___ Will this atom gain or lose? __neither___ How many ? ___0____ What is its combining capacity? _0_____ Charge ? __0____ Atoms with C.C. =_0=_INERT (NOBLE)_ that is , they will not blow up! (or react at all!)
Example 2: Neon atomic # = _10____ mass = ___20__ #p = __10___ #n = __10___ #e = __10___ # valence e = __8___ Will this atom gain or lose? __neither___ How many ? ___0____ What is its combining capacity? _0_____ Charge ? __0____ Atoms with C.C. =_0=_INERT (NOBLE)_ that is , they will not blow up! (or react at all!)
Now go back and answer the questions on the Bohr diagram
worksheets!
Now go back and answer the questions on the Bohr diagram
worksheets!
Charge:
Atoms are neutral if #p+ = # e- If atoms gain or lose electrons they
become _charged = IONS!_.
Charge:
Atoms are neutral if #p+ = # e- If atoms gain or lose electrons they
become _charged = IONS!_.
When naming NON-METAL ions, _change__ the name _ending_ to “_ide___”
e.g. _oxygen___ = __oxide_______ __fluorine___ = _fluoride
When naming NON-METAL ions, _change__ the name _ending_ to “_ide___”
e.g. _oxygen___ = __oxide_______ __fluorine___ = _fluoride
Non-metals form _negative ions. (_#e- > #p+)
Metals form _positive_ ions. (_#e- < #p+)
Non-metals form _negative ions. (_#e- > #p+)
Metals form _positive_ ions. (_#e- < #p+)
Study for Bohr Diagrams Quiz!
Study for Bohr Diagrams Quiz!
Recommended
