Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 1. Fill in the following tables. Symbol # # protons electrons # neutrons Atomic number Mass Number Atomic Mass Charge 56 54 83 18 16 32 35 47 1 19 40 1+ 92 241 0 Symbol # # protons electrons # neutrons Atomic number Mass Number Atomic Mass Charge 26 30 3+ 38 38 88 25 31 0 17 35 1 88 126 4+
Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 2. The following mixtures of isotopes are found in nature. Calculate the expected molar mass of a sample of each mixture. a) 10 B = 18.8%, 11 B = 81.2% b) 69 Ga = 60.0%, 71 Ga = 40.0% c) 70 Ge = 20.5%, 72 Ge = 27.4%, 73 Ge = 7.8%, 74 Ge = 36.5%, 76 Ge = 7.8% d) 90 Zr = 51.5%, 91 Zr = 11.2%, 92 Zr = 17.1%, 94 Zr = 17.4%, 96 Zr = 2.8%
Funsheet 8.1 [BOHR DIAGRAMS] Gu 2015 1. Draw Bohr diagrams for the following atoms: Element Neutral Ion O N K C Mg
Funsheet 8.1 [BOHR DIAGRAMS] Gu 2015 2. Draw Bohr diagrams for the following ionic compounds: Compound Bohr Diagram LiF KBr CaF 2
Funsheet 8.3 [THE ENERGY LEVEL DIAGRAM] Gu 2015 Fill the orbitals with F electrons Fill the orbitals with Ca electrons Fill the orbitals with Br electrons How many electrons are in F? How many electrons are in Ca? How many electrons are in Br? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? What is the electron configuration? What is the electron configuration? What is the electron configuration?
Funsheet 8.3 [THE ENERGY LEVEL DIAGRAM] Gu 2015 Fill the orbitals with Kr electrons Fill the orbitals with Ti electrons Fill the orbitals with Ni electrons How many electrons are in Kr? How many electrons are in Ti? How many electrons are in Ni? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? How many shells have electrons? How many sub shells have electrons? How many orbitals have a single electron? How many orbitals have paired electrons? What is the electron configuration? What is the electron configuration? What is the electron configuration?
Date: Name: Period: Electron Configuration Patterns on the Periodic Table The periodic table is highly useful for a number of reasons, one of them being to make writing electron configurations easy. To discover exactly how it does that, complete this simple activity. 1. Go to http://www.ptable.com/ 2. Click the Orbitals tab at the top of the page. This will show you the electron configuration for any element you hover your mouse over. The puzzle: The periodic table below is missing all of its labels but three! Using the clues given and the website for electron configurations, can you figure out the rest of the labels? 1s 4s 4d How did you figure out the rest of the labels? What do the labels represent? Compare your labeled periodic table with the orbital energy level diagram. What do you notice?
Funsheet 8.4 8.6 [ELECTRON CONFIGURATION] Gu 2015 Atom Full Electron Configuration Core Notation P # of Valence e Ti Co Br Sr Ar K Cd Ca Xe Cs **Pb Ga Mn Zr Sr 2+ Br N 3+ Ti 2+ N 2 Mn 2+ Ge 4+ Fe 3+ Ge 2+ Sb 3+
Funsheet 8.7 [ATOMIC RADII] Gu 2015 1. What happens to the atomic radius as you go across a period? Explain. 2. What happens to the atomic radius as you go down a group? Explain. 3. What happens to the atomic radius of an atom that becomes an anion? Explain. 4. What happens to the atomic radius of an atom that becomes a cation? Explain. 5. For each of the following pairs, circle the atom that has the larger atomic radius a) Br As b) Br As c) Sr Mg d) Ca Cs e) Ne Xe f) C O g) Hg Cl h) S Cl i) Na + Mg 2+ j) Fe 2+ Fe 3+
Funsheet 8.8 [IONIZATION ENERGY] Gu 2015 1. What is ionization energy? 2. What happens to ionization energy as you go across a period? Why? 3. What happens to ionization energy as you go down a period? Why? 4. How does the first ionization energy compare with the second? 5. Arrange the following atoms in order of increasing ionization energy: Sr, Cs, S, F, As 6. Which of the following neutral atom electron configurations has the higher ionization energy? a) [Ar]4s 2 3d 10 4p 5 b) [Ar]4s 2 7. How does the ionization energy of metals relate to their reactivity?
Funsheet 8.8 [IONIZATION ENERGY] Gu 2015 8. For each of the following pairs, circle the element with the higher ionization energy. a) F b) S c) Br d) Ca e) Na O Se Ar K Sr
Funsheet 8.9 [ELECTRONEGATIVITY] Gu 2015 1. What is electronegativity? 2. How does electronegativity change moving across a period? 3. How does electronegativity change moving down a group? 4. For the following pairs, circle the element with the higher electronegativity. a) Cr b) Na c) F d) He e) Sr Zn K F N Ag 5. How does electronegativity for non metals relate to their reactivity?
Funsheet 8.10 [TYPES OF BONDS] Gu 2015 Classify each of the following molecules as ionic, covalent, or polar covalent. If the molecule is polar covalent, indicate any partial charges and dipoles. 1) HBr 2) Cl 2 3) LiCl 4) NaF 5) HI 6) F 2 7) CsCl 8) MgO 9) O 2 10) KBr 11) HF 12) N 2 13) FeS 14) CO
Funsheet 8.11 [LEWIS STRUCTURES] Gu 2015 Draw the Lewis structure for the following elements and compounds. K As Br Si Te Al Cl 2 CaO H 2 O
Funsheet 8.11 [LEWIS STRUCTURES] Gu 2015 C 3 H 8 C 2 H 4 CH 2 F 2 H 2 O 2 NF 3 SiF 4 LiBr PBr 5 MgS
Funsheet 8.12 [FORMAL CHARGES] Gu 2015 1. Assign formal charges to the following molecules. a) b) c) d) 2. Possible Lewis structures for the following compounds are given. Select the most stable structure. a) BF 3 b) CH 3 CONH 2 c) C 2 H 5 NO
Funsheet 8.12 [FORMAL CHARGES] Gu 2015 3. Analysis was done on a bottle of CH 2 O 2. It was discovered that the compound exists in three forms, but in varying abundances. Explain why the first structure is the most prevalent out of the three, while the second is the least.
Funsheet 8.13 [CHARGED & RESONANCE STRUCTURES] Gu 2015 Draw the Lewis structure for the following molecules. Include all resonance forms and formal charges. O 3 (Avoid drawing this as a triangle. Triangles are very strained and unstable.) CO 3 2 HSO 4 HCO 2 NO 3 HPO 3 2
Funsheet 8.14 [BOND ENERGY] Gu 2015 1. In each of the following pairs of ionic compounds, circle the one with the higher melting point and briefly explain your reasoning. a) NaF, NaI b) CsF, CsCl c) LiCl, CaCl 2 2. Which compound has a stronger carbon carbon bond, C 2 H 6 or C 2 H 2?