1. Chapter 20 Chemical Bonds
Physical Science

2. Chemical Bonds Answer In your Notes!!
What do you think a chemical bond is?
What does it consist of?

3. Chemical Bonds
Chemical bond  forces holding atoms together to form molecules and solids
The attraction is between e- of one atom to the nucleus of another atom
Electric in nature

4. Section 1 Stability in Bonding Combined Elements
Uncombined elements such as copper, sulfur and oxygen can chemically combine to form a compound when conditions are right
EX: Statue of Liberty coloring

5. Section 1 Combined Elements
When elements combine, the new compound has unique properties EX: Na + Cl = NaCl (table salt) Sodium is a soft, shiny metal that reacts violently w/ water Chlorine is a poisonous greenish-yellow gas

6. Section 1 Formulas
Chemical formula- shows elements a compound contains and the exact number of atoms of each element
Chemical symbols & numbers are shorthand for the elements and their amounts in a chemical formula
EX: H20 contains:
2 hydrogen atoms & 1 oxygen atom

7. Formula Examples H2SO4 How many hydrogen atoms are there?
How many sulfur atoms are there?
How many oxygen atoms are there?
SiO2
How many silicon atoms are there?

8. Review Questions Describe what a chemical formula tell you.
Describe how the properties of table salt (NaCl) are different from those of sodium (Na) and chlorine (Cl).

9. Noble Gases
To understand the stability of the noble gases, it is helpful to look at electron dot diagrams Electron dot diagrams show only the electrons in the outer energy level of an atom Notice that eight dots surround Kr, Ne, Xe, Ar, and Rn, and two dots surround He.

10. Outer Levels-Getting Their Fill
How do elements, trying to become stable, gain or lose its outer electrons? Elements gain, lose, or share electrons to become stable by combining with other atoms that also have partially complete outer energy levels Electron dot diagrams for sodium and chlorine.

11. Outer Levels-Getting Their Fill
Fewer than 4 e-  give up e-
*More than 4 e-  gain e-
*4 e-  will try to share e- with another element
*Want 8 e- in the outer shell!

12. Stability is Reached
When atoms gain, lose, or share electrons, an attraction forms between the atoms, pulling them together to form a compound This attraction is called a chemical bond

13. Bellwork 2. What is a chemical bond? 3. Why are Noble Gases stable?
1. Why do elements form compounds?
2. What is a chemical bond?
3. Why are Noble Gases stable?
4. List the 3 ways bonds can be formed.
Write in your notes

14. Answers
To become more chemically stable by getting a complete outer energy level
The force that holds atoms together in a compound
Because they have a full outer energy level
Electrons are gained, lost or shared

15. Section 2 Types of Bonds Gain or Loss of Electrons
An atom that has lost or gained electrons is called an ion.
An ion is a charged particle
What do you think happens to the charge of an atom if it loses an electron?
What do you think happens to the charge of an atom if it gains an electron?

16. Section 2 Types of Bonds Gain or Loss of Electrons
Atom loses an electron, it becomes + ion.
a superscript indicates the charge
Atom gains an electron it becomes a − ion.

17. Section 2 Types of Bonds A Bond Forms
A neutral atom of potassium has one electron in its outer level. Is this a stable outer energy level? Why or Why not? When potassium forms a compound with iodine, potassium _____ one electron in it’s fourth level. What happens to the third level?

18. Section 2 Types of Bonds A Bond Forms
The potassium atom has become an ion.
When a potassium atom loses an electron, the atom becomes positively charged because there is one electron less in the atom than there are protons in the nucleus
The 1+ charge is shown as what?

19. Section 2 Types of Bonds A Bond Forms
The iodine atom in this reaction undergoes change, as well.
During the reaction with potassium, the iodide atom gains an electron, leaving its outer energy level with eight electrons. Is this considered stable?
This atom is no longer neutral because it gained an extra negative particle.
It now has a charge of 1 −

20. Section 2 Types of Bonds A Bond Forms
The resulting compound has a neutral charge because the positive and negative charges of the ions cancel each other.

21. Section 2 Types of Bonds Ionic Bond
Ionic bond- the force of attraction between opposite charges of the ions
In an ionic bond, a transfer of electrons takes place
If an element loses electrons, one or more elements must gain an equal number of electrons to maintain the neutral charge of the compound
Remember….
An ionic bond is usually formed between a ____ & ____
------ANSWER: METAL AND NONMETAL

22. Section 2 Types of Bonds Ionic Bond
Notice that Mg is losing 2 electrons and each of the Cl atoms is gaining 1 electron
What is lost is equally gained, therefore, the sum of the charges on the ions is zero

23. Section 2 Types of Bonds Sharing Electrons
For example, the elements in Group 14 of the periodic table have four electrons in their outer levels.
These atoms become more chemically stable by sharing electrons, rather than by losing or gaining electrons.

24. Section 2 Types of Bonds Covalent Bonds
The attraction that forms between atoms when they share electrons is known as a covalent bond
A neutral particle that forms as a result of electron sharing is called a molecule
Atoms can form double and triple bonds depending on whether they share two or three pairs of electrons

25. Section 2 Types of Bonds Polar or Nonpolar
A polar molecule has a slightly positive end and a slightly negative end, molecule is neutral. Water is an example of a polar molecule.
A nonpolar molecule is one in which electrons are shared equally in bonds.

26. Section 2 Discussion Questions
Write in your notes to help you study for the quiz!!
What is the sum of the charges when a compound is neutral?
Can atoms become more stable by sharing electrons?
A neutral particle that forms as a result of electron sharing is called a ________.
A single covalent bond is made up of how many electrons?

27. Answers 1). Zero (p. 610) 2). Yes ( p. 611) 3). molecule ( p. 611)
4). 2 shared electrons ( p. 611)

28. Section 3 Writing Formulas and Naming Compounds
Chemists use symbols from the periodic table to write formulas for compounds
Binary compound - compound composed of two elements
NOTE: Before you can write a formula, you need to know what the elements are and what number of electrons they GAIN, LOSE, or SHARE to be come stable.

29. Oxidation Numbers
Oxidation number- how many electrons an atom has gained, lost, or shared to become stable
In ionic compounds the oxidation number is the same as the charge of the ion
Elements can have more than one oxidation number

30. Determining Neutral Compounds
When writing a formula it is important to know that the compound is neutral (even thought the individual ions carry a charge)
The formula must have the right # of +ions and the right # of –ions so the charges balance
Use oxidation numbers or their least common multiples to write formulas
Use the name of the first element, the root name if the second element, and the suffix -ide to write the name of a binary compound

31. Examples of Neutral Compounds
NaCl (sodium chloride)
Sodium ion has a 1+ charge
Chlorine ion has a 1- charge
One of each ion makes this compound neutral

32. Examples of Neutral Compounds
CaF (calcium flouride)
Calcium ion has a 2+ charge
Flourine ion has a 1- charge
In this case you need to have 2 flourine ions for every calcium ion in order for the charges to cancel and the compound to be neutral.
Neutral formula = CaF2

33. Examples of Neutral Compounds
Example 3: AlO3 (Aluminum oxide) Aluminum ion has a charge of 3+ Oxygen ion has a charge of 2- Here you need to determine the least common multiple of 3 and 2 in order to determine how many ions of each you need. 6 is the least common multiple of these two numbers. You will need 2 aluminums and 3 oxygen ions to have a 6+ charge and a 6- charge for a neutral compound Neutral compound = Al2O3

34. Steps of Writing Formulas
Write the symbol of the element or polyatomic ion (ions containing more than one atom) that has the positive oxidation number.
Write the symbol of the element or polyatomic ion with the negative oxidation number.
The charge (without the sign) of one ion becomes the subscript of the other ion. Reduce the subscripts to the smallest whole numbers that retain the ratio of ions.

35. Steps of Writing Names for Binary Ionic Compounds
1. Write the name of the positive ion.
2. Check to see if the positive ion is
capable of forming more than one
oxidation number.
Write the charge of the positive ion
using roman numerals in parentheses
after the ion’s name if it has more than one oxidation number.

36. Steps to Writing Names for Binary Ionic Compounds
Write the whole first name of the first element.
Write the ‘root’ of the second element.
Add –ide or –ate.
Ex: Li Br
Lithium Bromide

37. Compounds with Added Water
Some ionic compounds have water molecules as part of their structure. These compounds are called hydrates.
A hydrate is a compound that has water chemically attached to its ions and written into its chemical formula.
When writing a formula that contains a hydrate, the number is shown after a “”. Following the number 2 is the formula for water as shown.

38. Steps for Naming Binary Covalent Compounds
Some pairs of nonmetals can form more than
one compound with each other.
Prefixes are used to indicate how
many atoms of each element are in a
binary covalent compound.
The last vowel of the prefix is
dropped when the second element begins
with a vowel as in pentoxide.
KNOW THESE PREFIXES

39. Using Prefixes
These same prefixes are used when naming the hydrates previously discussed.
The main ionic compound is named the regular way, but the number of water molecules in the hydrate is indicated by the Greek prefix.

40. Questions A binary compound is composed of two _____.
The net charge of a compound is ______.
A _______ is a compound that has water attached to its ions.
What prefix would be used for 7 atoms of one element in a covalent bond?
What is the 1st step in writing the formula for a binary ionic or binary compound formula?