Chapter 19—CHEMICAL BONDS

Chapter 19—CHEMICAL BONDS

Chapter 19 CHEMICAL BONDS Section 1Stability in Bonding Why is the Statue of Liberty Green? Copper, Sulfur, and Oxygen Some of the matter around you is in the

form of uncombined element, such as copper, sulfur, and oxygen. But, like many other sets of elements, these 3 elements unite chemically to form a compound when the conditions are right. The green coating on the Statue of Liberty and some old pennies is a result of this chemical change. Copper Sulfate (Copper + Sulfur + Oxygen) One

compound in this coating, is a new compound called copper sulfate. Copper sulfate isnt shiny and copper colored like elemental copper. Nor is it a pale-yellow solid like sulfur or a colorless, odorless gas like oxygen. Copper sulfate has its own unique properties. ExampleSodium + Chlorine = Salt (Sodium Chloride) SODIUM (SHINY, SOFT, SILVERY METAL)

CHLORINE (POISONOUS GREENISH-YELLOW GAS) Sodium(Na) + Chlorine(Cl) = Sodium Chloride(NaClChemical Formula) or Table Salt CHEMICAL FORMULA A chemical formula tells what elements

a compound contains and the exact number of atoms of each element in a unit of that compound. EXAMPLEH2O =CHEMICAL FORMULA H=hydrogen; O=oxygen; and a subscript of 2 = 2 atoms of hydrogen and if no subscript = 1 atom of oxygen ExampleBATTERY ACID OR SULFURIC ACID H2SO4 2 1 4

= hydrogen atoms sulfur atom oxygen atoms ATOMIC STABILITY Why do atoms form compounds? Atoms combine when the compound formed is more STABLE than the separate atoms. 115 elementsMOST combine with

other elements GROUP 18the 6 NOBLE GASES seldom form compounds. WHY? ATOMS OF GROUP-18 ARE UNUSUALLY STABLE These elements all have 8 electrons in their outer energy level, giving them a COMPLETE outer energy level. EXCEPT He only 2 electrons, but a COMPLETE outer energy level.

An atom is chemically stable (will not form compounds) when its outer energy level is COMPLETE. He = 2 outer electrons Ne = 8 outer electrons Ar = 8 outer electrons The Noble Gases are STABLE because they

each have a COMPLETE outer energy level. How do the ELECTRON DOT DIAGRAMS represent other elements? How does that relate to their ability to make compounds? HYDROGEN contains 1

electron in its 1 energy level. (INcomplete, UNstable) This is why so many hydrogen containing compounds, including WATER exist on Earth. HELIUM

In contrast, heliums outer energy level contains 2 electrons. Helium already has a full outer energy level by itself and is COMPLETE and STABLE. Helium rarely forms compounds, but, by itself, the element is a commonly used gas.

How does hydrogen or any other element find or get rid of extra electrons? Atoms with INcomplete outer energy levels can lose, gain, or share electrons to obtain a STABLE outer energy level. They do this by combining with other atoms that also have partially complete outer energy levels. RESULT: Each achieve stability. EXAMPLESODIUM AND

CHLORINE Sodium--GROUP 1 1 electron in its outer energy level (INCOMPLETE, UNSTABLE) ChlorineGROUP

17 7 electrons in its outer energy level (INCOMPLETE, UNSTABLE) SODIUM AND CHLORINE When these atoms combine, sodium loses 1 electron and chlorine gains 1 electron.

RESULT: Sodium and chlorine both receive a COMPLETE and STABLE outer energy level. EXAMPLEHYDROGEN AND OXYGEN

In the compound water, each hydrogen atom needs 1 electron to fill its outer energy level. The oxygen atom needs 2 electrons for its outer energy level to be stable with 8 electrons. HYDROGEN and OXYGEN share electrons instead of gaining or losing

electrons. WATER H2O When atoms gain, lose, or share electrons, an attraction forms between the atoms, pulling them together to form

a compound. This attraction or force that holds atoms together is a CHEMICAL BOND. Chapter 19: CHEMICAL BONDS Section 2TYPES OF BONDS What is an ION? An atom that has LOST or GAINED

electrons is called an ion. An ion is a charged particle, because it now has either MORE or LESS ELECTRONS than protons. The POSITIVE and NEGATIVE charges are NOT BALANCED. BEFORE (INDIVIDUAL ELEMENTS): PROTONS = ELECTRONS NOW (GETTING READY TO FORM COMPOUNDS):

PROTONS ELECTRONS EXAMPLE---NaCl (SALT) Some of the most common compounds are made by the LOSS and GAIN of just 1 ELECTRON. (Group 1 element + Group 17 element) Ex. NaCl ExamplesSodium chloride (table salt); sodium fluoride (anticavity ingredient in toothpaste); and potassium iodide (ingredient in

iodized salt) NaCL What happens when sodium and fluorine atoms come together? Na LOSES AN ELECTRONNa+ (1 LESS ELECTRON = POSITIVE CHARGE) The 1+ charge is shown as a superscript written AFTER the elements symbol, Na+, to indicate its charge. F GAINS AN ELECTRON F (1 MORE ELECTRON = NEGATIVE CHARGE) RESULT: The compound has a neutral charge,

because positive and negative charges of the ions cancel each other. Ex. NaF (Another Ex. Na+ and Cl- NaCl ) The IONIC Bond An ionic bond is a force of attraction between the opposite charges of the ions in an ionic compound. (Metal + Nonmetal) Ionic bond with more than 1 electron

involved MgCl2 MagnesiumGroup 2 and ChlorineGroup 17 When magnesium reacts with chlorine, a magnesium atom LOSES 2 electrons and becomes a POSITIVE charged ion, Mg2+. At the same time, 2 chlorine atoms GAIN 1 electron each and become NEGATIVE charged ions, Cl-.

A MAGNESIUM atom has 2 electrons to LEND, but a single CHLORINE atom needs to BORROW only 1 electron. Therefore, it takes 2 chlorine atoms to take the 2 electrons from the 1 magnesium ion. MgCl2 (Compound is neutral ) Magnesium LOSES 2 electrons = Mg2+ 2 Chlorine atoms

GAIN 2 electrons = ClCl(Each Cl atom GAINS 1 electron) MgCl2 ZERO NET CHARGE The POSITIVE CHARGE of the 1 magnesium ion is exactly EQUAL to the NEGATIVE CHARGE of the 2 chloride ions.

***Therefore, the compound is NEUTRAL. ***Ionic bonds usually are formed by bonding between METALS and NONMETALS (losing/gaining electrons). SHARING ELECTRONS Some atoms of NONMETALS are unlikely to LOSE or GAIN electrons. For example, the elements in GROUP 14 have 4 electrons in their outer energy level. They would have to lose or gain 4 electrons in order to have a stable outer energy level.

The loss of this many electrons takes a great deal of energy. Each time an electron is removed, the nucleus holds the remaining electrons even more tightly. COVALENT BOND

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. O = 6 electrons H = 1 electron H = 1 electron

2 SINGLE COVALENT BONDS COVALENT BONDS (N2, O2) N = 5 electrons N = 5 electrons ***3 pairs of electrons represent 3 bonds O = 6 electrons O = 6 electrons ***2 pairs of

electrons represent 2 UNEQUAL SHARING Electrons are not always shared equally between atoms in a covalent bond. The strength of the attraction of each atom ot its electrons is related to

SIZE of the atom CHARGE of the nucleus TOTAL NUMBER OF ELECTRONS the atom contains This type of molecule is called polar. A polar molecule is one that has a slightly positive end and a slightly negative end, although the overall charge is NEUTRAL. A nonpolar molecule is one in which electrons are shared equally in bonds. C = 4 electrons Cl = 7 electrons

***4 Chlorine atoms needed to equally share electrons, so that carbon and chlorine all have 8 electrons in their outer energy levels. CCl4 This type of molecule does not have oppositely charged

Chapter 19CHEMICAL BONDS Section 3WRITING FORMULAS AND NAMING COMPOUNDS WRITING FORMULAS The first formulas of compounds you will write are for binary ionic compounds. A

binary compound is a compound that is composed of 2 elements. EXAMPLEPotassium iodide, the salt additive, is a binary ionic compound. WRITING FORMULAS What do you need to know before you can write the formula? 1. Which ELEMENTS are involved?

2. What NUMBER OF ELECTRONS are lost, gained, or shared? (IN ORDER TO BECOME STABLE) OXIDATION NUMBER = CHARGE OF THE ION An OXIDATION NUMBER tells you how many electrons an atom has GAINED,

LOST, or SHARED to become stable. (p. 588) For ionic compounds, the OXIDATION NUMBER is the same as the CHARGE OF THE ION. EXAMPLESodium (Na) and Chlorine (Cl) CHARGE Na ion = Cl ion =

OX. # 1 + 1+ 1 - 1- Na = G-1, 1 outer electron (LOSES 1 ELECTRON OR LOSES 1 NEG CHARGE IS POS) Cl = G-17, 7 outer electrons (GAINS 1 ELECTRON OR GAINS 1 NEG CHARGE IS NEG) COMPOUNDS ARE NEUTRAL

Although the individual IONS in a compound carry CHARGES, the COMPOUND itself is NEUTRAL. ***A formula must have the right number of POSITIVE IONS and the right number of NEGATIVE IONS so the charges BALANCE. EXAMPLESodium chloride (NaCl) Na+ 1+ Cl1 0 (Compound is neutral/0 charge) CALCIUM FLUORIDE

Ca2+ = 2+ F1= 1In this case, you need to have 2 fluoride ions for every calcium ion in order for the charges to cancel and the compound to be NEUTRAL.

Ca F 2+ + 12+ + 2(1-) 2+ + 2- =0 (COMPOUND IS NEUTRAL) 1 ATOM OF Ca and 2 ATOMS OF F; CaF2 Aluminum Oxide Al3+ = 3+ O2- = 2What is the least common multiple of

3 and 2? 6 (2 x 3) 2 Al ions and 3 O ions are needed in order to have a 6+ charge and a 6charge IONS CHARGES Al= 2 x

3+ = 6+ O= 3 x 2= 60 Therefore, the nuetral compound = Al2O3 RULES FOR WRITING FORMULASSodium Chloride 1.

2. Write the symbol of the element or polyatomic ion (ions with more than 1 atom)that has a positive oxidation number or charge. Ex. Na ***H, ammonium ion (NH4), and all metals have positive oxidation numbers. Ex. Na = metal = + Write the symbol of the element or polyatomic ion with the negative oxidation number. Ex. Cl ***Nonmetals (other than H) and polyatomic ions (other than NH4) have negative oxidation

numbers. Ex. Cl = nonmetal = - RULES FOR WRITING FORMULAS(CONTINUED) 3. Use subscripts next to each ion so that the sum of the charges is ZERO. CHARGE Na ion =

1+ Cl ion = 1- Ex. Therefore, 1 atom of sodium and 1 atom of chlorine is neededNaCl COMPOUNDS WITH COMPLEX IONS Not all compounds are binary (contain 2 elements). Baking soda,

used in cooking, has the formula: NaHCO3 Which 4 elements does it contain? Na = sodium H = hydrogen C = carbon O = oxygen Some compounds, including baking soda, are composed of more than 2 elements. They contain polyatomic ions. poly = many

polyatomic = many atoms A polyatomic ion is a positively or negatively charged covalently (nonmetals) bonded group of atoms. RULES FOR WRITING NAMES

BaF2 1. You can name a binary ionic compound (2 elements1 metal and 1 nonmetal) (Using TABLE 2p.588, check to see if the positive ion is capable of forming more than

1 oxidation number.) Write the name of the positive RULES FOR WRITING NAMES (CONTINUED) Write the root name of the negative ion (NONMETAL). The root is the first part of the elements name. (chlorine = chlor-; oxygen = ox) Ex. Fluorine = fluor 3. Add the ending ide to the root. Ex. BaF2 = Barium fluoride 2.

RULES FOR WRITING NAMES POLYATOMIC IONSEx. NaHCO3 1. 2. The polyatomic ion in baking soda is the hydrogen carbonate ion.

(HCO3-) To name a compound that contains one of these ions Write the name of the positive ion (METAL). Ex. Sodium Write the name of the negative ion (NONMETALS) TABLE 4P.591Hydrogen carbonate (Sodium hydrogen POLYATOMIC IONEX.

K2SO4 Potassium sulfate WRITING FORMULAS FOR COMPOUNDS CONTAINING POLYATOMIC IONS, FOLLOW THE RULES FOR BINARY COMPOUNDS, WITH 1 ADDITION. ***When more than 1 polyatomic ion is needed, write parentheses around them before adding the subscript

EXAMPLEBARIUM CHLORATE Ba2+ ClO31 Ba ClO3 _____________________ 2+ 11 (2+) + 2(1-) (2+) + (2-) = 0 Ba(ClO3)2

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