1 Dalton’s Atomic Theory (1808) 1. Elements are composed of extremely small particles called atoms. 2. All atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of one element are different from the atoms of all other elements. 3. Compounds are composed of atoms of more than one element. In any compound, the ratio of the numbers of atoms of any two of the elements present is either an integer or a simple fraction. 4. A chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in their creation or destruction. Molecules, Atoms, and Ions

2 8 X 2 Y 16 X8 Y + Law of Conservation of Mass Molecules, Atoms, and Ions

3 atomic radius ~ 100 pm = 1 x m nuclear radius ~ 5 x pm = 5 x m Rutherford’s Model of the Atom “If the atom is the Houston Astrodome, then the nucleus is a marble on the 50-yard line.” Molecules, Atoms, and Ions

4 mass p ≈ mass n ≈ 1840 x mass e - Molecules, Atoms, and Ions

5 Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Isotopes are atoms of the same element (X) with different numbers of neutrons in their nuclei X A Z H 1 1 H (D) 2 1 H (T) 3 1 U U Mass Number Atomic Number Element Symbol Atomic Number, Mass Number, and Isotopes Molecules, Atoms, and Ions

6 The Isotopes of Hydrogen Molecules, Atoms, and Ions

Give the number of protons, neutrons, and electrons in each of the following species: (a) (b) (c) (d) carbon-14 Molecules, Atoms, and Ions

Solution (a) The atomic number is 11, so there are 11 protons. The mass number is 20, so the number of neutrons is 20 − 11 = 9. The number of electrons is the same as the number of protons; that is, 11. (b) The atomic number is the same as that in (a), or 11. The mass number is 22, so the number of neutrons is 22 − 11 = 11. The number of electrons is 11. Note that the species in (a) and (b) are chemically similar isotopes of sodium. Molecules, Atoms, and Ions

(c) The atomic number of O (oxygen) is 8, so there are 8 protons. The mass number is 17, so there are 17 − 8 = 9 neutrons. There are 8 electrons. (d) Carbon-14 can also be represented as 14 C. The atomic number of carbon is 6, so there are 14 − 6 = 8 neutrons. The number of electrons is 6.

10 The Modern Periodic Table Period Group Alkali Metal Noble Gas Halogen Alkali Earth Metal Molecules, Atoms, and Ions

11 Chemistry In Action Natural abundance of elements in Earth’s crust: Natural abundance of elements in human body: Molecules, Atoms, and Ions

12 A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical forces. H2H2 H2OH2ONH 3 CH 4 A diatomic molecule contains only two atoms: H 2, N 2, O 2, Br 2, HCl, CO A polyatomic molecule contains more than two atoms: O 3, H 2 O, NH 3, CH 4 diatomic elements Molecules, Atoms, and Ions

13 An ion is an atom, or group of atoms, that has a net positive or negative charge. cation – ion with a positive charge If a neutral atom loses one or more electrons it becomes a cation. anion – ion with a negative charge If a neutral atom gains one or more electrons it becomes an anion. Na 11 protons 11 electrons Na + 11 protons 10 electrons Cl 17 protons 17 electrons Cl - 17 protons 18 electrons Molecules, Atoms, and Ions

14 A monatomic ion contains only one atom: A polyatomic ion contains more than one atom: Na +, Cl -, Ca 2+, O 2-, Al 3+, N 3- OH -, CN -, NH 4 +, NO 3 - Molecules, Atoms, and Ions

15 Common Ions Shown on the Periodic Table Molecules, Atoms, and Ions

16 Formulas and Models Molecules, Atoms, and Ions

17 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance. An empirical formula shows the simplest whole-number ratio of the atoms in a substance. H2OH2O H2OH2O molecularempirical C 6 H 12 O 6 CH 2 O O3O3 O N2H4N2H4 NH 2 Molecules, Atoms, and Ions

Write the empirical formulas for the following molecules: (a)acetylene (C 2 H 2 ), which is used in welding torches (b)glucose (C 6 H 12 O 6 ), a substance known as blood sugar (c)nitrous oxide (N 2 O), a gas that is used as an anesthetic gas (“laughing gas”) and as an aerosol propellant for whipped creams. Molecules, Atoms, and Ions

(a)There are two carbon atoms and two hydrogen atoms in acetylene. Dividing the subscripts by 2, we obtain the empirical formula CH. (b)In glucose there are 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms. Dividing the subscripts by 6, we obtain the empirical formula CH 2 O. Note that if we had divided the subscripts by 3, we would have obtained the formula C 2 H 4 O 2. Although the ratio of carbon to hydrogen to oxygen atoms in C 2 H 4 O 2 is the same as that in C 6 H 12 O 6 (1:2:1), C 2 H 4 O 2 is not the simplest formula because its subscripts are not in the smallest whole-number ratio. (c) Because the subscripts in N 2 O are already the smallest possible whole numbers, the empirical formula for nitrous oxide is the same as its molecular formula. Molecules, Atoms, and Ions

20 Ionic compounds consist of a combination of cations and anions. The formula is usually the same as the empirical formula. The sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero. The ionic compound NaCl Molecules, Atoms, and

21 The most reactive metals (green) and the most reactive nonmetals (blue) combine to form ionic compounds. Molecules, Atoms, and Ions

22 Formulas of Ionic Compounds Al 2 O 3 2 x +3 = +63 x -2 = -6 Al 3+ O 2- CaBr 2 1 x +2 = +22 x -1 = -2 Ca 2+ Br - Na 2 CO 3 2 x +1 = +21 x -2 = -2 Na + CO 3 2- Molecules, Atoms, and Ions

Write the formula of magnesium nitride, containing the Mg 2+ and N 3− ions. When magnesium burns in air, it forms both magnesium oxide and magnesium nitride. Molecules, Atoms, and Ions

Solution To satisfy electrical neutrality, the following relationship must hold: (+2)x + (−3)y = 0 Solving, we obtain x/y = 3/2. Setting x = 3 and y = 2, we write Check The subscripts are reduced to the smallest whole- number ratio of the atoms because the chemical formula of an ionic compound is usually its empirical formula. Molecules, Atoms, and Ions

25 Chemical Nomenclature Ionic Compounds –Often a metal + nonmetal –Anion (nonmetal), add “-ide” to element name BaCl 2 barium chloride K2OK2O potassium oxide Mg(OH) 2 magnesium hydroxide KNO 3 potassium nitrate Molecules, Atoms, and Ions

26 Transition metal ionic compounds-indicate charge on metal with Roman numerals FeCl 2 2 Cl - -2 so Fe is +2iron(II) chloride FeCl 3 3 Cl - -3 so Fe is +3iron(III) chloride Cr 2 S 3 3 S so Cr is +3 (6/2)chromium(III) sulfide Molecules, Atoms, and Ions

27 Molecules, Atoms, and Ions

28 Molecules, Atoms, and Ions

2.5 Name the following compounds: (a)Cu(NO 3 ) 2 (b)KH 2 PO 4 (c)NH 4 ClO 3 Molecules, Atoms, and Ions

Solution (a)The nitrate ion ( ) bears one negative charge, so the copper ion must have two positive charges. Because copper forms both Cu + and Cu 2+ ions, we need to use the Stock system and call the compound copper(II) nitrate. (b)The cation is K + and the anion is (dihydrogen phosphate). Because potassium only forms one type of ion (K + ), there is no need to use potassium(I) in the name. The compound is potassium dihydrogen phosphate. (c) The cation is (ammonium ion) and the anion is. The compound is ammonium chlorate. Molecules, Atoms, and Ions

Write chemical formulas for the following compounds: (a)mercury(I) nitrite (b)cesium sulfide (c)calcium phosphate Molecules, Atoms, and Ions

(a)The Roman numeral shows that the mercury ion bears a +1 charge. According to Table 2.3, however, the mercury(I) ion is diatomic (that is, ) and the nitrite ion is. Therefore, the formula is Hg 2 (NO 2 ) 2. (b)Each sulfide ion bears two negative charges, and each cesium ion bears one positive charge (cesium is in Group 1A, as is sodium). Therefore, the formula is Cs 2 S. (c) Each calcium ion (Ca 2+ ) bears two positive charges, and each phosphate ion ( ) bears three negative charges. To make the sum of the charges equal zero, we must adjust the numbers of cations and anions: 3(+2) + 2(−3) = 0 Thus, the formula is Ca 3 (PO 4 ) 2. Solution Molecules, Atoms, and Ions

33 Molecular compounds −Nonmetals or nonmetals + metalloids −Common names −H 2 O, NH 3, CH 4 −Element furthest to the left in a period and closest to the bottom of a group on periodic table is placed first in formula −If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom −Last element name ends in -ide Molecules, Atoms, and Ions

34 HIhydrogen iodide NF 3 nitrogen trifluoride SO 2 sulfur dioxide N 2 Cl 4 dinitrogen tetrachloride NO 2 nitrogen dioxide N2ON2Odinitrogen monoxide Molecular Compounds Molecules, Atoms, and Ions

Name the following molecular compounds: (a)SiCl 4 (b)P 4 O 10 Molecules, Atoms, and Ions

Strategy We refer to Table 2.4 for prefixes. In (a) there is only one Si atom so we do not use the prefix “mono.” Solution (a)Because there are four chlorine atoms present, the compound is silicon tetrachloride. (b)There are four phosphorus atoms and ten oxygen atoms present, so the compound is tetraphosphorus decoxide. Note that the “a” is omitted in “deca.” Molecules, Atoms, and Ions

Write chemical formulas for the following molecular compounds: (a)carbon disulfide (b) disilicon hexabromide Molecules, Atoms, and Ions

Strategy Here we need to convert prefixes to numbers of atoms (see Table 2.4). Because there is no prefix for carbon in (a), it means that there is only one carbon atom present. Solution (a)Because there are two sulfur atoms and one carbon atom present, the formula is CS 2. (b) There are two silicon atoms and six bromine atoms present, so the formula is Si 2 Br 6. Molecules, Atoms, and Ions

39 Molecules, Atoms, and Ions

CHAPTER 3 PERIODIC TABLE Classification of the elements into periods, groups and blocks. Metals and Non-metals

41 The Modern Periodic Table Period Group Alkali Metal Noble Gas Halogen Alkali Earth Metal Molecules, Atoms, and Ions

Classification of the Elements Periodic Table

Cations and Anions Of Representative Elements Periodic Table

CHAPTER 4 CHEMICAL BONDING Types of Chemical Bonding: Ionic Bonding and Covalent Bonding

Ionic Bonds metal to nonmetal metal loses electrons to form cation nonmetal gains electrons to form anion ionic bond results from + to – attraction –larger charge = stronger attraction –smaller ion = stronger attraction Ionic bond: the electrostatic force that holds ions together in an ionic compound. Chemical Bonding

Li + F Li + F - The Ionic Bond 1s 2 2s 1 1s 2 2s 2 2p 5 1s 2 1s 2 2s 2 2p 6 [He][Ne] Li Li + + e - e - + FF - F - Li + + Li + F - LiF Lewis Theory allow us to predict the correct formulas of ionic compounds Chemical Bonding

Covalent Bonds often found between two nonmetals typical of molecular species atoms bonded together to form molecules –strong attraction sharing pairs of electrons to attain octets molecules generally weakly attracted to each other –observed physical properties of molecular substance due to these attractions Chemical Bonding

A covalent bond is a chemical bond in which two or more electrons are shared by two atoms. Why should two atoms share electrons? FF + 7e - FF 8e - Chemical Bonding