1. Atoms, Molecules and Ions Chapter 2

2. Dalton’s Atomic Theory (1808) 1. ____________ are composed of extremely small particles called atoms. All atoms of a given element are identical. The atoms of one element are different from the atoms of all other elements. 2. ____________ are composed of atoms of more than one element. The relative number of atoms of each element in a given compound is always the same. 3. _______________ involve only the rearrangement of atoms—atoms are not created or destroyed in chemical reactions. 2.1

3. 2 Law of _________________________________

4. 8 X 2 Y 16 X8 Y + 2.1 Law of _________________________________

5. J.J. Thomson, measured mass/charge of e - (1906 Nobel Prize in Physics) 2.2 A = alpha B = gamma C = beta

6. e - charge = -1.60 x 10 -19 C Thomson’s charge/mass of e - = -1.76 x 10 8 C/g e - mass = 9.10 x 10 -28 g Measured mass of e - (1923 Nobel Prize in Physics) 2.2

7. (Uranium compound) 2.2

9. 1.atoms positive charge is concentrated in the nucleus 2.proton (p) has opposite (+) charge of electron 3.mass of p is 1840 x mass of e - (1.67 x 10 -24 g)  particle velocity ~ 1.4 x 10 7 m/s (~5% speed of light) (1908 Nobel Prize in Chemistry) 2.2

10. atomic radius ~ 100 pm = 1 x 10 -10 m nuclear radius ~ 5 x 10 -3 pm = 5 x 10 -15 m Rutherford’s Model of the Atom 2.2

11. Chadwick’s Experiment (1932) H atoms - 1 p; He atoms - 2 p mass He/mass H should = 2 measured mass He/mass H = 4  + 9 Be 1 n + 12 C + energy neutron (n) is neutral (charge = 0) n mass ~ p mass = 1.67 x 10 -24 g 2.2

12. Subatomic Particles (Table 2.1, p.36) mass p = mass n = 1840 x mass e - 2.2

13. _______________ (Z) = number of protons in nucleus ______________(A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons ___________ are atoms of the same element (X) with different numbers of neutrons in the nucleus X A Z H 1 1 H (D) 2 1 H (T) 3 1 U 235 92 U 238 92 Mass Number Atomic Number Element Symbol 2.3

15. How many protons, neutrons, and electrons are in C 14 6 ? How many protons, neutrons, and electrons are in C 11 6 ? Do You Understand Isotopes? 2.3

16. Period Group Alkali Metal Noble Gas Halogen Alkali Earth Metal 2.4

17. ____________ is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds H2H2 H2OH2ONH 3 CH 4 A __________ molecule contains only two atoms H 2, N 2, O 2, Br 2, HCl, CO A _________ molecule contains more than two atoms O 3, H 2 O, NH 3, CH 4 2.5

18. An ____ is formed when an atom, or group of atoms, has a net positive or negative charge (why?). _____ – ion with a positive charge If a neutral atom _______ one or more electrons it becomes a cation. _____ – ion with a negative charge If a neutral atom _______ 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 2.5

19. A __________ ion contains only one atom A __________ ion contains more than one atom 2.5 Na +, Cl -, Ca 2+, O 2-, Al 3+, N 3- OH -, CN -, NH 4 +, NO 3 -

20. Do You Understand Ions? 2.5 How many protons and electrons are in Al 27 13 ? 3+3+ How many protons and electrons are in Se 78 34 2- ?

21. 2.5

22. 2.6

23. A ___________ formula shows the exact number of atoms of each element in the smallest unit of a substance An ____________ 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 2.6

24. ______ compounds consist of a cation and an anion the formula is always the same as the empirical formula the sum of the charges on the cation and anion in each formula unit must equal zero The ionic compound NaCl 2.6

25. Formula of Ionic Compounds Al 2 O 3 2.6 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 1 x +2 = +21 x -2 = -2 Na + CO 3 2-

26. Some Polyatomic Ions 2.7

27. Chemical Nomenclature Ionic Compounds –often a metal + nonmetal –anion (nonmetal), add “ide” to element name BaCl 2 K2OK2O Mg(OH) 2 ___________________ KNO 3 2.7 ___________________

28. Transition metal ionic compounds –indicate charge on metal with Roman numerals FeCl 2 2 Cl - -2 so Fe is +2 _________________ FeCl 3 3 Cl - -3 so Fe is +3 Cr 2 S 3 3 S -2 -6 so Cr is +3 (6/2) 2.7 _________________

29. Molecular compounds –nonmetals or nonmetals + metalloids –common names H 2 O, NH 3, CH 4, C 60 –element further left in periodic table is 1 st –element closest to bottom of group is 1 st –if more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom –last element ends in -ide 2.7

30. HI NF 3 ___________________ SO 2 N 2 Cl 4 NO 2 N2ON2O Molecular Compounds 2.7 TOXIC ! Laughing Gas ___________________ _______________ ___________________

31. An _______ can be defined as a substance that yields hydrogen ions (H + ) when dissolved in water. HCl Pure substance, hydrogen chloride Dissolved in water (H + Cl - ), hydrochloric acid An ___________ is an acid that contains hydrogen, oxygen, and another element. HNO 3 ________________ H 2 CO 3 ________________ H 2 SO 4 ________________ 2.7

33. A ________ can be defined as a substance that yields hydroxide ions (OH - ) when dissolved in water. NaOH ______________ KOH _________________ Ba(OH) 2 _________________ 2.7