Unit 3 Review

1. Unit 3 Review Chemistry

2. 1. Label the periodic groups #1 Alkali Metals # 2Alkaline Earth Metals # 8 Noble Gases # 7 Halogens Transition Metals

3. 2. Circle the most EN element and square the least EN element3. Highest IE red and lowest IE blue Small atoms! High IE and EN Highest EN Lowest IE LARGE atoms, low IE and EN

4. 5. Number the periods6. Shade period 4 blue7. The rows are periods and the columns are _______________ groups 1 2 3 4 5 6 7 increasing atomic # 8. The periodic table is organized by_______________

5. 9. Use arrows to show the trend for increasing atomic size/radius. Circle the atom with the largest size/radius.

6. Metals (red – for review wksht) Nonmetals (blue for review wksht) Metalloids (green – for review worksheet)

7. Alkali metals – group 1 11) Have 1 valence electron ____________________ 12) Have 8 valence electrons ____________________ 13) Have 7 valence electrons ____________________ 14) Have 2 valence electrons Noble Gases – group 18 Halogens – group 17 Alkaline Earth metals – Group 2

8. Noble Gases 15) The least reactive elements ____________________ 16) The most reactive nonmetals (gases at room temperature)___________________ 17) The most reactive metals ____________________ 18) Reacts explosively with oxygen and water ____________________ 19) Used to make coins and jewelry. Halogens Alkali metals Alkali Metals Transition Metals

9. Ionization Energy 20) Energy required to remove an electron from an atom____________________ 21) The ability of atom to attract electrons. 22) List 3 other elements that will have similar chemical properties to Nitrogen and explain why. Electronegativity Most like: Phosphorus (P) 2nd most like: Arsenic (As) 3rd most like: Antimony (Sb) Same group –gives them same # of valence electrons and ion charge, therefore similar reactivity!

10. Circle the element in the pair has the larger ionization energy. Explain why. a. Li, N b. Kr, Ne c. Cs, Li Explain the octet rule. Circle the element in the pair is more electronegative. Explain Why? a. K, As b. N, Sb c. Sr, Be Closer to Fluorine! Atoms will lose, gain, or share electrons to have 8 valence electrons in their outer energy level. Smaller atoms – less shielding – nucleus charge is stronger and can attract the electron more easily.

11. Periodic law states that elements show a a. repetition of their physical properties when arranged by increasing atomic radius. b. repetition of their chemical properties when arranged by increasing atomic radius. c. periodic repetition of their properties when arranged by increasing atomic number. d. periodic repetition of their properties when arranged by increasing atomic mass.

12. Elements in the same group of the periodic table have the same: • number of valence electrons • physical properties • number of electrons • Which of the following is NOT true of an atom, other than Helium, obeying the octet rule? • a. obtains a full set of 8 valence electrons • b. acquires the valence electrons of a noble gas • c.possess 8 electrons in total • d. has a s2p6 valence configuration

13. Moving down the periodic table, which two atomic properties follow the same trend? a. atomic radius, ionization energy b. atomic radius, electronegativity c. ionization energy, electronegativity d. none of the above Which will form a larger ionic radii than its’ parent atom? a. cation (+ ion) b. anion (- ion) Explain your choice! Extra electrons cause repulsion and cloud spreads out – ion gets bigger!

14. 8 total 23) How many electrons does an atom of Oxygen have? _____ How many valence electrons?________ How many electrons does 0-2 have? _____ 24) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why fluorine holds on to its electrons so well) 6 10 total, 8 valence NUCLEAR/positive

15. 1s2 2s2 2p6 3s2 3p6 4s2 25) Which element is this for? ____________________- 26) In which period is this element found in?______ In which group #? _______ 27) How many electrons are in this element’s 3rd energy level? _____ 28) Re-write the electron configuration of this element if it became an ion with a +2 charge Calcium 4 2 8 1s2 2s2 2p6 3s2 3p6 It loses the 2 electrons in 4s

16. Cloud Shaped Electron 29) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found. 30) How many orbitals (circles) are in each sublevel? a. S = ___ b. P = ___ c. d = ___ d. F = ____ 31) How many electrons can fit into 1 orbital? _____ 3 1 5 7 2 electrons

17. 32) Is the following electron sketch correct? Explain 3s 3p 4s 3d It is not correct, the 3d orbitals should have one in each orbital and then it should double up!

18. 33) Label the following blocks

19. p 34) Identify the blocks where these groups are found – a. Halogens = ____ block b. Alkaline Earth Metals = _____ block c. Alkali Metals = ______ block d. Rare Earth Metals = ______ block e. The Noble Gases = _____ block f. The Transition Metals = _______ block s s f p d

20. 35) Identify the spectrum A: Hydrogen & Helium B: Helium, Barium, Sodium C: Barium, Calcium, Hydrogen, Helium

21. Photons and the Electromagnetic Spectrum 36) An electron that is closest to the nucleus possible (at the lowest energy level possible) is said to be in its ___________ _________________. 37) When an electron jumps up to a higher energy level and then falls back to its ground state a ___________ is released. Ground State Photon

22. Photons and the Electromagnetic Spectrum 38) The amount of energy released by an electron jumping from the 4th energy level back to its ground state at the 3rd energy level will always release a photon with a___________________________ (different-variable/specific-quantized) amount of energy. 39) The color spectra (types of colors produced) of a star can be used to identify the types of ______________ present in the star. Elements