1. Periodic Law Review Chapter 5

2. This man organized the periodic table by increasing atomic mass. This man organized the periodic table by increasing atomic number. The definition of periodic law is… Dmitri Mendeleev Henry Moseley Physical and chemical properties are periodic functions of their atomic numbers.

3. Periodic functions means…. The name of the first family. The name of the second family. A repeating trend because of.. Alkali metals Alkaline Earth Metals

4. The name of the 2 nd to last family. The name of the last family. This family all ends in s 2 Halogens Noble Gases Alkaline Earth Metals

5. This family ends in p 6 This family ends in s 1 This family ends in p 5 Noble Gases Alkali Metals Halogens

6. These three families are highly reactive. This family is relatively unreactive. This family gains 1e- when bonding. Alkali metals, halogens, and alkaline earth metals Noble gases halogens

7. This family loses 1 e- when bonding. This family loses 2e- when bonding. This family has a full s and p orbital in the principal energy level. Alkali metals Alkaline earth metals Noble gases

8. The definition of electronegativity… The trend across a period…. The trend down a family/group. The measure of the tendency of an atom to gain an electron from another atom. Electronegativity increases. Electronegativity decrease or remain the same.

9. The definition of electron affinity… The trend across a period…. The trend down a family/group. The energy change that occurs when an electron is acquired by a neutral atom. Electron affinity become more negative in the p block; becomes more positive going from group 1 to group 2. The energies become less.

10. The definition of ionization energy… The trend across a period…. The trend down a family/group. The energy required to remove one electron from a neutral atom of an element. Ionization energies of the main group elements increase across a period. Ionization energies of the main group generally decrease down a group.

11. The definition of atomic radius… The trend across a period…. The trend down a family/group. The average distance between two bonded atoms. Atomic radius decreases across a group. Atomic radius increases down a group.

12. The definition of ionic radii… The trend across a period…. The trend down a family/group. The average distance between 2 bonded atoms that are a cation or anion. Cationic radii decrease across a period. Anionic radii decrease across each period. Ionic radii (cationic and anionic) increase down a group.

13. The definition of valence electrons… The trend across a period…. The trend down a family/group. The number of electrons found in the outermost s and p orbitals. They are available to gain, lose or share. Valence electrons increase by 1 in the main group. Valence electrons remain the same in each family.

14. H V C Hydrogen Vanadium Carbon

15. O S U Oxygen Sulfur Uranium

16. F I Ne Fluorine Iodine Neon

17. Br Mg Ca Bromine Magnesium Calcium

18. Pt Ti Sn Platinum Titanium Tin

19. W Au Hg Tungsten Gold Mercury

20. Rn Fr Ar Radon Francium Argon

21. Sc Be Li Scandium Beryllium Lithium

22. How many atoms are in 1 mol? What is the above number referred to as? The number of protons is called? 6.022 x 10 23 Avogadro’s number Atomic number

23. The number of protons + neutrons is called? Atoms of the same element which differ in the number of neutrons are called? The average mass taking into account the abundance of all of the isotopes of that element is called? Mass number isotopes Atomic mass (that’s why it is a decimal on the periodic table.

24. How do you obtain the mass number when all you are given on the periodic table is atomic number and atomic mass? The element [He] 2s 2 The element [Kr] 5s 1 Rounding the atomic mass to the nearest whole number will give you the mass number of the most common isotope. Be Rb

25. The electron configuration for K. The electron configuration for C. The electron configuration for Kr. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 1s 2 2s 2 2p 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6

26. The noble gas configuration for P. The noble gas configuration for As. The noble gas configuration for Ne. [Ne]3s 2 3p 3 [Ar]4s 2 3d 10 4p 3 [He]2s 2 2p 6

27. Convert 4.0mol O to atoms of O. Convert 25.0 x 10 23 atoms S to mol S. Convert 14.0 g Mg to mol Mg. 4.0 mol O x 6.022 x 10 23 atoms =2.4 x 10 24 1 mol O 25.0 x 10 23 atoms S x 1 mol =4.15 mol S 6.022 x 1023 atoms 14.0 g Mg x 1 mol Mg =.576 mol Mg 24.30 g Mg

28. Convert 14.0 g of O to mol O. Convert 10.0 g of Au to atoms Au. Convert 5.0 g S to atoms of S. 14.0 g O x 1 mol =.875 mol O 16.0 g O 10.0 g Au x 6.022 x 1023 atoms Au =3.06 x 10 22 196.97 g Au 5.0 g S x 6.022 x 10 23 atoms S = 9.4 x 10 22 atoms S 32.065 g S