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7.1 Compounds, Atoms and Ions Date:
Warm up:
Study Notes/Questions Atoms vs Compounds
Atoms
_________________ particle of an element
over ______________________________
about ___________________________________
Compounds
simplest particle = __________________________
elements combined _______________________
new substances ‐‐> ________________________
many ___________________of compounds
How Atoms Form Compounds
bonding based on ______________________________________
want _____________________________ (valence shells) with same # of
__________________________________
halogens tend to __________________________________
alkali metals tend to __________________________________
Atoms vs Ions
Atom ‐ neutral ‐ same number _____________________________ Ion ‐ charged particle
‐ different ___________________________________ ‐ has __________________________ 1 or more electrons
Note: Any element can be an atom or an ion
Fluorine Atom vs Fluorine Ion
7.1 Compounds, Atoms and Ions
Study Notes/Questions E.g. Draw a Magnesium Ion
Ion Properties
Symbols
Use element symbols with charge _______________________
E.g.
Non‐metal ion names _____________________________
Transferring Electrons
Atoms become ____________________________ with full shells
Can’t do it on their own, but ___________________________
Result: ________________________________
Note: ________________________________________
Predicting Ion charge from Periodic Table
____________________________ alkali metals (group 1) 1+ , alkaline earth (group 2) 2+
______________________________ halogens (group 17) 1‐
______________________________ 1+ or 1‐
Summary: (two to three sentences summarizing this section)
Self‐Reflection Questions:
1. Describe one thing that you knew about this topic before today.
2. Describe one thing you learned about this topic today.
7.1 Activity
1. Write a definition of a compound. Include three points in your definition.
2. How does a compound’s properties compare to those of its component elements? Provide an example.
3. What is a valence electron?
4. Draw Bohr diagrams of the following:
(a) O and O2- (b) Mg and Mg2-
(c) Be and Be2- (d) N and N3-
5. Complete the following table. Note that the name of a NON-METALLIC ion ends in -IDE while the name for a METALLIC ion uses the full name of the metal.
ION NAME
ION SYMBOL
NUMBER OF
PROTONS
NUMBER OF ELECTRONS
NUMBER OF ELECTRONS
LOST OR GAINED
SAME # OF
ELECTRONS AS WHAT
NOBLE GAS?
ex
fluoride
1
53
54
2
16
gained two
3
potassium
lost one
4
Ca2+
5
35
36
6
Sr2+
7
H+
(none)
8
8
gained two
9
12
lost two
10
aluminium
10
11
34
36
12
H -
13
lithium
lost one
14
Rb+
15
17
18
7.2 Chemical Bonding Date:
Warm up:
Study Notes/Questions Chemical Bonding
A ________________________ is a force that holds atoms together to form
__________________________.
There two types: __________________________
Ionic Bonds: Metal + Non-Metal
__________________ valence electrons
strong attraction of ______________________________
Ex. CaF2
Note:
Covalent bonds: Non-metal + Non-metal
________________________ valence electrons between atoms
forms __________________________________ (basic unit is a molecule)
For example
Each atom has _____________________________
7.2 Chemical Bonding
Study Notes/Questions Diatomic Atoms Explained
By pairing up, both atoms _________________ Remember, they form the "7"
Properties of Ionic compounds
Strong __________________________
_________________ alternating + and – ions
Definite _______________________________
High _________________________
_______________ and _________________________
Conduct electricity when ___________________________
Properties of Molecular (Covalent) compounds Crystals have ______________________________
_____________________________________ (and boiling points)
_________________________________ when dissolved in H2O (do not separate into ions)
Type of Substance Smallest Particle
Summary: (two to three sentences summarizing this section)
Self-Reflection Questions:
1. Describe one thing that you knew about this topic before today.
2. Describe one thing you learned about this topic today.
7.2 Activity
1. What do we call a physical force that holds atoms together?
2. Explain the difference between an ionic bond and a covalent bond.
3. Draw Bohr diagrams of a magnesium atom bonding with fluorine atoms. Draw atoms, then
electron transfer, and finally the ions that form. What type of bonding occurs?
4. Draw Bohr diagrams of two hydrogen atoms bonding with an oxygen atom by sharing
electrons to form a water molecule. What type of bonding occurs?
5. Explain why the melting points of ionic compounds and molecular compounds differ.
7.2 Activity
6. Explain why an ionic compound is hard and brittle.
7. (a) What laboratory procedure allows you to test if a compound is ionic or molecular?
(b) What results would you expect?
8. (a) What do we call the smallest particle of an element?
(b) What do we call the smallest particle in a compound with ionic bonds?
(c) What do we call the smallest particle of a covalently bonded compound?
7.3 Part 1 ‐ Ionic Compounds: Chemical Formulas and Naming Date:
Warm up:
Study Notes/Questions Chemical Formula
shorthand method of ___________________________________________
_______________________________ of the component elements
Total ion charge = _____________________________
Binary Ionic Compounds
ionic compounds with ________________________________
Positive ion (metal ion) _____________________, negative ion ________________
Use ______________________to show numbers of each element needed
Formulas for Binary Ionic Compounds
1. Need symbol and ion charge 2. Balance ion charges to complete formula.
E.g. 1) Calcium combining with oxygen
2) potassium with nitrogen 3) Aluminum with sulfur
Binary Compounds with Multivalent Elements
______________________ – can form ions with more than one charge (transition metals)
You will be told which one to use in each situation
E.g. Copper can be + 1 or +2
Manganese (III) and sulfur
7.3 Part 1 ‐ Ionic Compounds: Chemical Formulas and Naming
Study Notes/Questions Ionic Compounds: Naming
The chemical names are derived ____________________________________________. Remember non‐metal ion names __________________________________________. For example: For multivalent metals use _________________________ to show the charge on the ion
Cu+ and O2‐ =
Mn3+ and S2‐ =
Determine the chemical formula from the name
E.g. Sodium Nitride
If you know the formula, work backwards to find the metal ion charge
Example: SnO2
Summary: (two to three sentences summarizing this section)
Self‐Reflection Questions:
1. Describe one thing that you knew about this topic before today.
2. Describe one thing you learned about this topic today.
7.3 Activity Part 1: Binary Ionic Compounds
Combine Ions and Charges Formula Name
Calcium and
Chlorine
Magnesium and
Nitrogen
Potassium and
Oxygen
Aluminum and
Sulphur
Beryllium and
Bromine
Lead (II) and
Silicon
Copper (I) and
Phosphorus
Zinc and Oxygen
Mercury (II) and
Iodine
Iron (III) and
Nitrogen
Calcium and
Fluorine
Barium and
Carbon
Silver and
Oxygen
Iron (II) and
Iodine
E. Write either the chemical formula or chemical name for these binary ionic compounds:
(a) strontium sulfide
(b) CaCl2 (c) lithium bromide
(d) K2O
(e) beryllium oxide
(f) Li2Se
(g) potassium phosphide
(h) Ca3N2
(i) calcium arsenide
(j) MgF2
(k) scandium oxide
(l) Na2S
(m) magnesium oxide
(n) ZnCl2
(o) sodium nitride
F. Write either the chemical formula or chemical name for these ionic compounds with multivalent
elements: (a) molybdenum(III) sulphide
(b) PbCl2
(c) rhodium(IV) bromide
(d) Cu2O
(e) mercury(II) oxide
(f) Tl2Se
(g) bismuth(V) phosphide
(h) PbF4
(i) rhenium(VII) arsenide
(j) CoF2
(k) copper(I) telluride (l) Fe2S3
(m) niobium(V) iodide
(n) PtBr4
(o) titanium(IV) nitride
7.3 Part 2 ‐ Ionic Compounds: Chemical Formulas and Naming Date:
Warm up: Determine the chemical formula for E.g. Sodium Nitride
E.g. Lithium Oxide
E.g. Magnesium Phosphide
Determine the chemical name for E.g. Fe2S3
E.g. AuI3
E.g. TiN
Study Notes/Questions Ionic Compounds with Polyatomic Ions Polyatomic Ions ‐ certain atoms that bond together first and then act as a single ion
E.g. 1) Sodium Carbonate
2) Tin (IV) Phosphate
3) Potassium Acetate
Summary: (two to three sentences summarizing this section)
Self‐Reflection Questions:
1. Describe one thing that you knew about this topic before today.
2. Describe one thing you learned about this topic today.
7.3 Part 2 Activity
1. Write either the chemical formula or chemical name for these ionic compounds with polyatomic ions:
(a) sodium acetate
(b) PbCrO4 (c) barium acetate
(d) CaSO4
(e) mercury(II) chlorite (f) Li3PO4
(g) bismuth(V) phosphate
(h) (NH4)2HPO4
(i) rhenium(VII) permanganate
(j) Co(ClO4)2
(k) copper(II) hydrogen oxalate
(l) Fe2(SO4)3
(m) chromium(II) hydrogen sulphide
(n) Ba(ClO)2
(o) titanium(IV) nitrite
2. First classify each of the following ionic compounds as binary, multivalent, or polyatomic (combinations
can exist). Then write either the chemical formula or chemical name.
(a) potassium acetate
(b) PbF2
(c) calcium acetate
(d) Li2O
(e) copper(II) chlorite
(f) Na3PO4
(g) lithium phosphide
(h) (NH4)2SO4
(i) rhenium(VII) nitride
(j) CaCl2
(k) lead(II) hydrogen oxalate
(l) Cr2S3
(m) iron(II) hydrogen sulfide
(n) PbBr4
(o) tin(IV) nitride
7.4 Molecular Compounds: Chemical Formulas and Naming Date: Warm up:
Study Notes/Questions Molecular Compounds: Chemical Formulas and Naming
__________________________________ ‐ non‐metal atoms share electrons to bond. Atoms combine in ____________________________________________________ e.g. Chemical formulas for molecular compounds come from ________________________ (and vice versa) based on a _____________________________ Formulas: ______________________________________________________ Names: add prefix according ___________________________________________
(omit “mono” on first element only) Formula: Name:
Some molecular compounds have __________________________________________________
dihydrogen monoxide
nitrogen trihydride
carbon tetrahydride
Summary: (two to three sentences summarizing this section)
Self‐Reflection Questions:
1. Describe one thing that you knew about this topic before today.
2. Describe one thing you learned about this topic today.
7.4 Activity: Molecular Compounds: Formula Writing and Naming
Write either the chemical formula or chemical name for these molecular compounds: (a) nitrogen monoxide
(b) SiO2 (c) boron monoxide
(d) P2O5
(e) tellurium dibromide (f) CO2
(g) dinitrogen tetraoxide
(h) SeF2 (i) carbon disulfide
(j) AsBr4
(k) arsenic trioxide (l) S2O5
(m)sulfur dioxide
(n) CS2 (o) tetraphosphorus decaoxide