Unit 3 Review Honors Chemistry

2-Alkaline Earth Metals 1-Alkali Metals 18- Noble Gases 17-Halogens 3-12 Transition Metals

High IE and EN Small atoms! High IE and EN Highest IE Highest EN Lowest IE

Organized by increasing atomic number 1 2 3 4 5 6 7

Atomic Radius Trends Smaller across period – higher nuclear charge Bigger down- More energy levels!

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

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

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

19) Energy required to remove an electron from an atom ____________________ 20) The ability of atom to attract electrons. 21) List 3 other elements that will have similar chemical properties to Nitrogen and explain why. Ionization Energy Electronegativity Phosphorus, Arsenic and Antimony Same group –gives them same # of valence electrons and ion charge, therefore similar reactivity!

22. Circle the element in the pair has the larger ionization energy 22. Circle the element in the pair has the larger ionization energy. Explain why. a. Li, N b. Kr, Ne c. Cs, Li 23. Explain the octet rule. 24. Circle the element in the pair is more electronegative. Explain Why? a. K, As b. N, Sb c. Sr, Be Smaller atoms – have less shielding – higher nuclear charge to hold on to its valence electrons! Atoms will lose or gain 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.

25. 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. 26. Elements in the same group of the periodic table have the same: a. number of valence electrons b. physical properties c. number of electrons 27. 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

a. atomic radius, ionization energy 28. 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!

30) How many electrons does an atom of Oxygen have? _____ How many electrons does 0-2 have? _____ 31) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why fluorine holds on to its electrons so well) 8 total, 6 valence electrons 10 total, 8 valence NUCLEAR

1s2 2s2 2p6 3s2 3p6 4s2 3d6 32) Which element is this for? ____________________- 33) In which period is this element found in?______ In which group #? _______ 34) How many electrons are in this element’s 3rd energy level? _____ 35) Re-write the electron configuration of this element if it became an ion with a +2 charge Fe - Iron 4 8 14 1s2 2s2 2p6 3s2 3p6 3d6 It loses the 2 electrons in 4s d-orbitals do not change!

38) How many electrons can fit into 1 orbital? _____ 36) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found. 37) How many orbitals are in each sublevel? a. S = ___ b. P = ___ c. d = ___ d. F = ____ 38) How many electrons can fit into 1 orbital? _____ Cloud Shaped Electron 1 3 5 7 2 electrons

39) What do the quantum numbers tell us about an atomic orbital? The probable location of an electron The main energy level it is on. The shape of the orbital (s, p, d or f) it is in. The orientation of that orbital around the nucleus The spin direction of the electron

40) Is the following orbital notation for the 3rd and 4th energy levels of the element in #32 above 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!

#40

41) 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 p s s f p d

Photons and the Electromagnetic Spectrum 41) An electron that is closest to the nucleus possible (at the lowest energy level possible) is said to be in its ___________ _________________. 42) When an electron jumps up to a higher energy level and then falls back to its ground state a ___________ is released. Ground State Photon

Photons and the Electromagnetic Spectrum 43) 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. 44) The color spectra (types of colors produced) of a star can be used to identify the types of ______________ present in the star. Elements