science 10 chemistry notes what is 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:
- anything that has __________________ and takes up __________________.
- Is the make up of the entire universe.
- Is made up of atoms and elements.
Periodic Table of the Elements
Metals: Found to the _____________ of the “ladder”.
Generally shiny ______________ at room temperature and
_______________ conductors of heat and electricity.
Non-Metals: Found to the ____________ of the
“ladder”. Exist in all three states of matter,
___________, and ____________ conductors.
Metalloids: Found along ______________________ of
the ladder. Have properties of ___________ metals and
non-metals.
Horizontal rows are called ______________________.
Vertical columns are called _______________ or
________________.
Periodic Table Analogy Lab
How to Read the Periodic Table:
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Anatomy of an Atom Element: A _____________ substance that ______________ be broken down
into a simpler substance (made up of ____________________ kind of atom).
Atom: the basic unit of an ______________________.
Let’s determine which element this is:
How many electrons?
_____________________
How many valence electrons? ______________
How many protons? ______________________
How many neutrons? _____________________
Atomic number = number of protons = __________
Atomic mass = # protons + # neutrons = ______________
Element Symbol Atomic
#
Atomic
Mass
Protons
p+
Neutrons
n0
Electrons
e-
Cesium
Selenium
Bromine
Assignment: How to Count Protons, Neutrons and Electrons
Bohr Diagrams of Atoms Neils Bohr developed a theory to identify where ____________________ are found
around the nucleus (Hotel Analogy)
e- surround the nucleus in _______________/ _____________/_________________
1st Ring can hold max ____ e- 2nd Ring can hold max _____e- 3rd Ring can hold max ______e-
Ex) Na atom (____________ e-) ex) Sulfur atom (____________ e-)
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Assignment: Bohr Diagram Periodic Table Worksheet
How Atoms Become Stable (p+≠ e-)
Electrons in the outermost ring are called ____________________________
When outermost shell is full, element is ________________
Atoms may gain or lose ___________________________ in order to get a full valence shell,
thus becoming _______________ (charged particles).
Ex) Sodium atom Outer shell has ______ electron Sodium ION
P+ = e- = P+ = e- =
Ex) Fluorine atom Outer shell has ______ electron Fluoride ION
P+ = e- = P+ = e- =
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 ______
gain _____
b) Nitrogen
lose ______
gain _____
Assignment: Atom/Ion Worksheet
- Only _____________________________ 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 ______________________
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 (_____________________)
- If an atom gains an electron, it becomes a negative ion (____________________)
Determining p+, n0, e- of Ions
Ions ≠ Neutral # ______________ ≠ # ____________
Ex) Li1+ atomic # = p+= no = e- =
Ca2+ O2-
p+ 16 13
no
e- 18 10
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 _______________, giving up
or __________________ 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 _______________ bond with ________________.
2. Covalent Compounds: where _________________ bond with other __________________.
1. Ionic Compounds Ex) Sodium + Chlorine Here we see that sodium (______________) will give its
valence electron to chlorine (_________________) so that
they both have stable shells.
Once this happens, the ionic charge of sodium will be _____
and the ionic charge of chlorine will be ____.
These two opposing charges will attract each other and a
chemical bond will be formed creating the compound
__________________.
Sometimes, more than one electron can be transferred.
Ex) Magnesium + Oxygen
This compound’s name is __________________________.
Sometimes more than one atom of each element will have to be involved.
Ex) Beryllium + Fluorine
This compound’s name is ___________________________.
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____________________
Aluminum chloride___________________
Calcium phosphide ___________________
Lithium nitride_____________________
Potassium selenide ___________________
c) 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
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3. Transition Metal Ionic Compounds (M + NM)
a) Writing Formulas (Name Formula)
Copper (II) sulfide _____________________
Copper (I) sulfide ____________________
iron (III) oxide _____________________
mercury (II) phosphide ___________________
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 ______________________________ PbO2 ______________________________
CoS _____________________________ Co2S3 _____________________________
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- NO33-
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
Understanding Concepts
In your own words, explain what is meant by the term “polyatomic ion”. Give 2
examples.
1. 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 ______________________________________________
2. P2O3 _______________________________________________
3. CF4 _______________________________________________
4. SO2 _______________________________________________
5. N2O ______________________________________________
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 _______________
2. disilicon hexabromide _______________
3. diarsenic trioxide _______________
4. selenium monosulfide _______________
5. carbon tetrabromide _______________
6. boron trifluoride _______________
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Understanding Concepts
1. How can you tell the difference between an ionic compound and a molecular
compound?
2. What kinds of atoms form molecular compounds?
3. How do the atoms in molecular compounds form stable electron arrangements?
In other words, what happens to the 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, covalent, and mixed naming
2. 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
o 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:
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:
Draw 2-pentanol and 3-pentanol
Assignment: Naming Alcohols
Practice Exam/Review
EXAM