Science 10 Chemistry Notes What is Chemistry?mrsmaier.wikispaces.com/file/view/Science 10 Chemistry...
Transcript of Science 10 Chemistry Notes What is Chemistry?mrsmaier.wikispaces.com/file/view/Science 10 Chemistry...
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Science 10 – Chemistry Notes Name: _________________
What is Chemistry? Chemistry is the science in which substances are examined to find out:
- What things are made of
- How they act under different conditions
- How they are combined or separated to form other substances.
Essentially, chemistry is the study of ___matter____.
Matter:
- anything that has ____mass______ and takes up ____space____.
- Is the make up of the entire universe.
- Is made up of atoms and elements.
Periodic Table of the Elements
Metals: Found to the __left__ of the “ladder”. Generally
shiny ___solids__ at room temperature and
___good____ conductors of heat and electricity.
Non-Metals: Found to the ___right__ of the “ladder”.
Exist in all three states of matter, __dull__, and
___poor__ conductors.
Metalloids: Found along ___both sides____ of the
ladder. Have properties of ___both___ metals and non-
metals.
Horizontal rows are called ____periods____.
Vertical columns are called ___groups____ or ____families_____.
Periodic Table Analogy Lab
How to Read the Periodic Table:
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Anatomy of an Atom Element: A __pure___ substance that ___cannot___ be broken down into a simpler
substance (made up of ___the same__ kind of atom).
Atom: the basic unit of an __element (of matter)___.
Let’s determine which element this is:
How many electrons? ______6__
How many valence electrons? ___4______
How many protons? ______6______________
How many neutrons? _____6______________
Atomic number = number of protons = ___6_____
Atomic mass = # protons + # neutrons = ___12_
Element Symbol Atomic
#
Atomic
Mass
Protons
p+
Neutrons
n0
Electrons
e-
Cesium
Cs 55 133 55
133-55
=78 55
Selenium
Se 34 79 34
79-34
= 45 34
Bromine
Br 35 80 35
80-35
= 45 35
Assignment: How to Count Protons, Neutrons and Electrons
Bohr Diagrams of Atoms Neils Bohr developed a theory to identify where ___electrons__ are found around the
nucleus (Hotel Analogy)
e- surround the nucleus in __orbits__/ __rings__/__energy levels_
1st Ring can hold max _2_ e- 2nd Ring can hold max _8_e- 3rd Ring can hold max _8_e-
Ex) Na atom (__11__ e-) ex) Sulfur atom (__16__ e-)
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Assignment: Bohr Diagram Periodic Table Worksheet
How Atoms Become Stable (p+≠ e-)
Electrons in the outermost ring are called ___valence electrons____
When outermost shell is full, element is __stable__
Atoms may gain or lose __ELECTRONS__ in order to get a full valence shell, thus becoming
____IONS__ (charged particles).
Ex) Sodium atom Outer shell has __1_ electron Sodium ION
Na1+
P+ = 11 e- = 11 p+ = 11 e- = 10
Ex) Fluoride atom Outer shell has __9_ electron Fluoride ION
F1-
P+ = 9 e- = 9 P+ = 9 e- = 10
Group Valence e- Lose or Gain
1 1 lose 1 gain 7
2 2 lose 2 gain 6
3/13 3 lose 3 gain 5
4/14 4 lose 4 gain 4
5/15 5 lose 5 gain 3
6/16 6 lose 6 gain 2
7/17 7 lose 7 gain 1
8/18 8 lose 8 gain 0
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Fill in the chart for the following:
Atom Bohr diagram for
atom
Bohr diagram for
stable ion
Gained/lost
electrons
Formula of
ION that is
formed
Same number of
electrons as what
Noble Gas?
a) Lithium
lose __1 e-___
gain _____
Li 1+
He
b) Nitrogen
lose ______
gain _3 e-_
N3-
Ne
Assignment: Atom/Ion Worksheet
- Only ____ELECTRONS__ can be gained or lost from an atom.
o The atomic number is different for every element on the periodic table of the
elements. It is characteristic for that element. You ___CANNOT____ change the
number of protons! If you change the number of protons, you change the atomic
number, and you have a different element!!
- If an atom loses an electron, it becomes a positive ion (__caTion__)
- If an atom gains an electron, it becomes a negative ion (__aNion__)
Determining p+, n0, e- of Ions
Ions ≠ Neutral # ____ p+___ ≠ # __e-___
Ex) Li1+ atomic # = p+= no = e- =
Ca2+ O2- S2- Cl1-
p+ 20 8 16 17
no 20 8 16 18
e- 18 10 18 18
Assignment: Determining Protons, Neutrons, and Electrons for Ions
Gold Penny Lab
In-Class Assignment: p+, n0, e- for atoms/ions; Bohr diagrams for atoms/ions,
gained/lost electrons, ion that’s formed, same Bohr diagram as what atom?
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How Elements Form Compounds In order for atoms to have a stable valence shell, they will link up with other atoms by ___gaining__, giving up or
____sharing__ electrons. This is how elements combine to form compounds.
There are two major types of compounds that can form between atoms:
1. Ionic Compounds: where ____metals___________ bond with ___non-metals_____.
2. Covalent Compounds: where ____non-metals____ bond with other __non-metals__.
1. Ionic Compounds Ex) Sodium + Chlorine Here we see that sodium (___metal__) will give its valence
electron to chlorine (__non-metal___) so that they both have
stable shells.
Once this happens, the ionic charge of sodium will be _Na1+_
and the ionic charge of chlorine will be _Cl1-_.
These two opposing charges will attract each other and a
chemical bond will be formed creating the compound __sodium
chloride (NaCl)___.
Sometimes, more than one electron can be transferred.
Ex) Calcium + Oxygen
This compound’s name is ____calcium oxide_____.
Sometimes more than one atom of each element will have to be involved.
Ex) Calcium + Chlorine
This compound’s name is ___calcium chloride___.
Assignment: Making Simple Ionic Compounds
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2. Simple Ionic Compounds (M + NM)
a) Writing Formulas (Ions→ formula)
Writing Formulas for Ionic Compounds
Look up the Symbol and Charge
left-hand side right hand side
metal and non-metal (or polyatomic)
Figure out how many of each element you need to make sure your charges cancel out
THE CHARGES GO AWAY BECAUSE YOUR PLUSES CANCEL YOUR MINUSES!!!!
ionic formula ionic formula
left-hand side right hand side left-hand side right hand side
sodium phosphide magnesium sulfide
Na1+ P3- I need 3 Na1+ Mg2+ S2- I need 1 Mg2+
Na1+ to cancel out P3- to cancel out 1
Na1+ Na3P S2-
MgS
Given the name, write the formula
Potassium bromide____KBr____
Aluminum chloride____AlCl3______
Calcium phosphide ___Ca3P2_____
Lithium nitride____Li3N_______
Potassium selenide ___K2Se____
b) Naming Simple Ionic Compounds ( M + NM) Formula → Name
ionic naming ionic naming
Na3P CaI2
left-hand side right hand side left-hand side right hand side
sodium phosphide calcium iodide
Ex) NaCl K2O CaF2
BaS2 Na3N Li3As
Assignment:
Naming Ionic
Compounds and
Writing Ionic
Formulas
Worksheet
sodium chloride potassium oxide
chloride
calcium fluoride
chloride
barium sulfide sodium nitride
chloride
lithium astetide
chloride
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3. Transition Metal Ionic Compounds (M + NM)
a) Writing Formulas (Name Formula)
Copper (II) sulfide _____CuS_______
Copper (I) sulfide ____Cu2S__________
iron (III) oxide _____Fe2O3_________
mercury (II) phosphide ______Hg3P2______
b) Naming (Formula Name)
MnCl2 Cu3N2
left-hand side right hand side left-hand side right hand side
manganese (II)? chloride copper (I)? nitride
OR manganese (III)? chloride OR copper (II)? nitride
Mn? Cl1- 2 minuses Cu? N3-
Cl1- Cu? N3-
Cu?
therefore must be Mn+2 so 1 Mn cancels therefore must be Cu+2 so 3 Cu cancels
with 2 Cl1- with 2 N3-
manganese (II) chloride copper (II) nitride
PbO ______lead (II) oxide__________ PbO2 ________lead (IV) oxide___________
CoS _____cobalt (II) sulfide_______ Co2S3 _____cobalt (III) sulfide_______
Assignment: Ionic Compounds: Metals with More than one Charge
4. Polyatomic Compounds
a) Writing Formulas (Name Formula)
ionic formula ionic formula
left-hand side right hand side left-hand side right hand side
sodium iodate gold (III) nitrate
Na1+ IO3- I need 1 Na1+ Au3+ NO3
1- I need 1 Au3+
to cancel out 1 IO3- NO3
1- to cancel out 3
NaIO3 NO3 1- NO3
3-
Au(NO3)
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sodium chlorite
barium nitrate
magnesium carbonate
calcium hydroxide
b) Naming (Formula Name)
Na3PO4 Ca(OH)2
left-hand side right hand side left-hand side right hand side
sodium phosphate calcium hydroxide
Name the following compounds:
Na2SO4 Al(ClO3)3 NH4NO3 Rb2HSO3
Assignment: Making Polyatomic Ionic Compounds Using Models Activity
Assignment: Polyatomic Compounds Names and Formulas Worksheet
5. Acids Are covalent compounds (electrons are SHARED) that give off hydrogen ions when dissolved in
water.
They ALWAYS start with H+ bonded to some negative ion (either a non-metal or a polyatomic ion).
There are three kinds of acids:
o Hydrogen bonding with an –ate ions
o Hydrogen bonding with an –ite ions
o Hydrogen bonding with an –ide ions
a) Writing Names (formula name) Naming Acids
If the anion ends in –ate, it is called ________ic acid
Ex) Hydrogen Nitrate, HNO3 ____nitric_____ acid
If the anion ends in –ite, it is called ________ous acid
Ex) Hydrogen Nitrite, HNO2 ____nitrous____ acid
If the anion ends in –ide, it is called hydro______ic acid
Ex) Hydrogen Chloride, HCl __hydrochloric_ acid
H+ and a polyatomic
H+ and a non-metal
(most of the
time…exceptions are
OH-, CN-)
sodium sulfate Aluminum chlorate
chloride
Ammonium nitrate
nitrate
astetide
chloride
rubidium hydrogen sulfite OR
rubidium bisulfite
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Practice: name the following acids.
1. HI _________________________ 4. H3P
2.
3.
Acid
Starts with H Ends with
-ide -ate -ite
(one symbol after the H)
hydro________ic acid __________ic acid __________ous acid
H2S H3BO3 H2CrO3
hydrogen selenide hydrogen borate hydrogen chromite
hydroselenic acid boric acid chromous acid
-IDE acids If there is only one symbol after the H, write “hydro”, then take the element’s name
and change the ending to “ic”. Ex) H2Se = hydroselenic acid
-ATE acids change the “ate” to say “ic” and say “acid”. Ex) H3BO3… BO3 is called borate. So call
this boric acid.
–ITE change the “ite” to say “ous” and say “acid”. Ex) H2CrO3… CrO3 is called chromite. So call
this chromous acid
b) Writing Formulas (name formula)
Use the same criss-cross method as with ionic compounds. H1+ will ALWAYS be at the
start of your criss-cross.
Writing Formulas for Acids hydro________ic acid ___________ic acid _______________ous acid
hydronitric acid nitric acid nitrous acid
hydrogen nitride hydrogen nitrate hydrogen nitrite
H1+ N3- I need 3 H1+ H1+ NO31- I need 1 H+1 H1+ NO2
1- I need 1H+
H1+ to cancel out to cancel out to cancel
H1+ N3- NO31- NO2
1-
H3N HNO3 HNO2
Examples:
Hydrosulfuric acid (H1+ and ) _________________
Carbonic acid (H1+ and ) _______________
Nitrous acid (H1+ and ) _______________
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Practice: write the formula for the following acids
1. chromic acid ____H2CrO4__
2. sulfurous acid____H2SO3_____
3. carbonous acid ____H2CO2____
4. hydrocyanic acid___HCN___
5. hydrochloric acid __HCl__
6. oxalic acid _____H2C2O4______
7. sulfuric acid ____H2SO4__________
8. chlorous acid _____HClO2_______
9. hydrosulfuric acid __H2S_____
10. boric acid ____H3BO3________
Assignment: Acids – Names and Formulas
Understanding Concepts
In your own words, explain what is meant by the term “polyatomic ion”. Give 2
examples.
many atoms with a charge – anything from the right hand side of the ion chart
11. Covalent (Molecular) Compounds (Non Metal/Non Metal)
Are formed when 2 NON-METALS bond
Here, electrons are SHARED, not transferred as they are in ionic compounds.
Naming: A prefix is used to indicate the number of each element in the compound. (The exception is we don’t use
mono- for the first element).
Charges are not of concern in covalent compounds.
Drop the ending of the second element and add –ide.
Examples: CCl4 carbon tetrachloride
N2O3 dinitrogen trioxide
Prefix Number
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10
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Practice: Name the following covalent compounds. 1. PBr3 ________phosphorus tribromide_______
2. P2O3 ________diphosphorus trioxide_________
3. CF4 __________carbon tetrafluoride________
4. SO2 _______silicon dioxide________
5. N2O _______dinitrogen monoxide_______
Writing Formulas Completely ignore the charges of the non-metals!!!
The prefixes will tell you how many atoms of each element you need.
DO NOT reduce compounds to lowest form! Leave them as the name states.
Examples: Nitrogen trihydride NH3
Dinitrogen tetraoxide N2O4
Practice: Write the formulas for the following covalent compounds.
1. tetraphosphorus triselenide ____P4Se3_____
2. disilicon hexabromide ____Si2Br6_____
3. diarsenic trioxide ____As2O3_____
4. selenium monosulfide ____SeO____
5. carbon tetrabromide ____CBr4______
6. boron trifluoride ____BF3________
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Understanding Concepts
1. How can you tell the difference between an ionic compound and a molecular
compound?
ionic – something from the right hand side and the left hand side
covalent – two things from the right hand side
2. What kinds of atoms form molecular compounds?
two non-metals
3. How do the atoms in molecular compounds form stable electron arrangements?
In other words, what happens to the electrons?
Molecular compounds SHARE electrons
Assignment: Covalent (Molecular) Compounds: Names and Formula Worksheet
BONUS: Mixed Ionic and Covalent Compounds
IN-CLASS ASSIGNMENT #2: Naming and Writing Formulas for ionic, metals with more than one
charge, polyatomic ions, acids, covalent, and mixed naming
12. Hydrocarbons: Alkanes and Alkenes
a) Alkanes An alkane is a saturated hydrocarbon. In other words, an alkane is a long chain of carbon linked
together by single bonds.
The general formula for alkanes is CnH2n+2.
Formula Structure
The simplest alkane is methane
Formula Structure
o The next simplest is ethane
o The series continues indefinitely
**Each C must have 4 bonds **
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Naming Alkanes Naming alkanes is quite simple: just use prefixes counting the number of carbon atoms in the
formula and add the suffix –ane.
The prefixes are as follows:
Examples:
NAME: butane hexane
Alkanes can be symbolized in a few different ways:
Molecular Formula Expanded structural Formula Condensed structural Formula
Ex) propane
b) Alkenes Alkenes are unsaturated hydrocarbons which means their carbon structure contains double bonds.
The general formula for alkenes is CnH2n
The simplest alkene is ethene (C2H4)
Naming Alkenes Naming alkenes is generally the same as naming alkanes, but with the suffix -ene and a
number indicating which carbon the double-bonded is attached to in the chain.
You can number the carbons either left to right or right to left. You must pick whichever
way gives the carbon with the double bond the LOWEST possible number.
Ethene and propene do not require numbers, since there is no question as to where the
double-bonded carbon is in the structures.
Example: propene C3H6
Example: butene C4H8 can have the double bonded
carbon in two different places. NAME:
NAME:
**Give the double bond the lowest
number **
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Assignment: Simple Alkanes and Alkenes
Naming Alcohols
Alcohols are organic carbons similar to alkanes but one of the hydrogen’s is substituted with a
hydroxide group, OH.
Alcohols are named by replacing the final –e of the alkane with the suffix “–ol”.
The location of the hydroxyl group is indicated with a number. The chain is numbered to give the
alcohol functional group the lowest possible number.
Example)
NAME: methanol ethanol 3-propanol 1-propanol 2-propanol
Draw 2-pentanol and 3-pentanol
2-pentanol 3-pentanol
Assignment: Naming Alcohols
Practice Exam/Review
EXAM