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Chapter 20 Chemical Bonds

Chapter 20 Chemical Bonds. Physical Science. Chemical Bonds. Answer In your Notes!! What do you think a chemical bond is? What does it consist of?. Chemical Bonds. Chemical bond  forces holding atoms together to form molecules and solids

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Chapter 20 Chemical Bonds

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  1. Chapter 20Chemical 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 BondingCombined 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 1Formulas 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. FormulaExamples • 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? • How many oxygen 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 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 BondsGain 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 BondsGain 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 BondsA 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 BondsA 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 BondsA 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 BondsA 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 BondsIonic 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 BondsIonic 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 BondsSharing 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 BondsCovalent 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 BondsPolar 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 EXAMPLE 1: 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 EXAMPLE 2: 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 Namesfor 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 NamingBinary 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?

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