7.1 compounds, atoms and ions date - wordpress.com

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


Self-Reflection Questions:



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





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

7.3 Activity Part 2: Naming Binary Ionic Compounds

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





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





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

7.1 compounds, atoms and ions date - wordpress.com

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