HONORS Chemistry Midterm Review

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Alberta Warner
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1 HONORS Chemistry Midterm Review This review sheet is a list of topics and sample practice problems only. The practice problems are good representation of what to expect on the midterm, but it is not enough to just study from the review. You need to look over your notes, old review sheets, tests and quizzes, homework, etc. Ask questions!!!! You may check your answers online and I am available Tuesday, Wednesday, and Fridays for extra help. Chapter 1 & 2: Intro to Chemistry What is chemistry Uncertainty in Measurement sig figs Physical and chemical properties Physical and chemical changes 1. Determine the number of significant figures in the following values: a c. 15,300 3 b d Perform the following calculations and express your answer with the correct number of significant figures: a x = 1550 b = -50. Chapter 3: Atomic Structure Models of the atom (Modern atomic theory) Isotopic Notation, Subatomic particles Atomic Orbitals s, p, d shapes Electron configurations Valence electrons Periodic Law 3. Describe the basic structure of the atom in the modern atomic theory (be able to label protons, neutrons, electrons, and the nucleus) (Ch. 3): Protons, neutrons in nucleus (densely packed) Electrons surrounding nucleus in orbitals/clouds Protons: + Electrons: - Neutrons: neutral

2 14 C 4. 6 protons = 6 neutrons = 8 electrons = 6 5. Sketch s and p orbitals (Ch 3): Electron clouds where there is a probability of finding electrons 6. Write the electron configuration for Bromine. 1s 2 2s 2 2p 6 3s 3 3p 6 4s 2 3d 10 4p 5 7. What element has the following electron configuration: 1s 2 2s 2 2p 6 3s 3 3p 6 4s 2 3d 5 Manganese Chapter 4: The Periodic Table Organization of the Periodic Table (Periodic Law) Periodic Trends: Electronegativity Recognize properties of main groups 8. State the periodic law (Ch 4): Elements are grouped on periodic table by their physical and chemical properties (atomic number increases). The physical and chemical properties of the elements are periodic functions of their atomic numbers (pg 116).

9. Label the following areas on your periodic table (some may overlap) (Ch 4): Chapter 5: Ionic Compounds Octet Rule Naming and writing formulas Properties of ionic versus covalent compounds 10.

dissolved in water Both form stable octets (8 valence electrons) Both do not conduct electricity as solids Nonmetal & nonmetal Sharing of electrons Low MP and BP Poor conductors of electricity 11.

3 9. Label the following areas on your periodic table (some may overlap) (Ch 4): Chapter 5: Ionic Compounds Octet Rule Naming and writing formulas Properties of ionic versus covalent compounds 10. Compare and contrast ionic and covalent bonds (Ch 5 and 6, essay): Ionic Both Covalent Metal & nonmetal Giving/taking electrons (transferring) High MP and BP Conducts electricity when molten or dissolved in water Both form stable octets (8 valence electrons) Both do not conduct electricity as solids Nonmetal & nonmetal Sharing of electrons Low MP and BP Poor conductors of electricity 11. Name the following ionic formulas (Ch 5): a. NH 4 Cl Ammonium chloride b. CuO Copper(II) oxide c. NaF Sodium fluoride d. Mg(NO 3 ) 2 Magnesium nitrate 12. Write formulas for the following ionic compounds (Ch 5): a. Magnesium Hydroxide Mg(OH) 2 b. Copper(II) Chloride CuCl 2 c. Calcium Hydroxide Ca(OH) 2 d. Sodium Phosphate Na 3 PO 4

4 Chapter 6: Covalent Compounds Topics: Naming and writing formulas Properties Lewis Dot structures Polar vs. Non-polar covalent bonds VSEPR Be able to Sketch lewis structures and predict molecular geometries (VSEPR) 11. Name the following covalent compounds (Ch 6): a. CO 2 Carbon dioxide b. SiF 4 Silicon tetrafluoride c. SnO 4 Tin tetraoxide d. CCl 4 Carbon tetrachloride 12. Write formulas for the following covalent compounds (Ch 6): a. dinitrogen pentoxide N 2 O 5 b. phosphorus trichloride PCl 3 c. carbon monoxide CO d. selenium hexachloride SeCl Write the dipole moment and bond character of each (Ch 6): a. C-H =.4 nonpolar covalent b. C-S =0 nonpolar covalent c. Na-Cl =2.3 ionic d. Si-O =1.5 polar covalent e. Cl-N =.2 nonpolar covalent 14. Draw Lewis Structures (Ch 6): CH 3 Cl OF 2 SO 3 Check answers during class.

5 15. Identify the shape and bond angle of molecular compounds (Ch 6): Lewis Structure Shape Bond angles NH 3 Trigonal pyramidal <109.5 SO 2 Linear 180 CCl 4 Tetrahedral Chapter 7: Organic Chemistry Topics: Organic bonding Hydrocarbons Alkanes, alkenes, alkynes Naming and drawing formulas Functional groups Practical applications 16. Define hydrocarbon: compounds containing carbon and hydrogen atoms 17. Compare/Contrast Alkanes, Alkenes, Alkynes: Type of Bonds Name Alkane Single -ane Alkene Double -ene Alkyne Triple -yne 18. List and describe 3 uses of organic compounds (Ch 7, organic presentations) Soap, perfumes, synthetic fabrics, polymers, medicine, PLASTIC petroleum (energy)

6 19. Drawing and naming organic structures and naming (Ch 7): Recognize how to draw/name structures for alkanes, alkenes, and alcohols. 3-octene Pentane 1-butanol 2-pentene

7 Chapter 8: The Mole Topics: Mole Avogadro s number Percent composition Empirical formulas Molecular formulas Be able to Calculate molar mass Convert between grams and moles Convert between number of particles and moles Perform multi-step conversions Calculate percent composition Determine empirical formula Determine molecular formula 20. Determine the molar mass of the following compounds (Ch 8): Al 2 (SO 4 ) 3 2(26.98) + 3(32.06) + 12(16.00) = KBr Li 2 O = g/mol 2(6.94) = 29.88g/mol 21. Find the percent composition of each element (Ch 8): %Mg in MgSO 4? Total mass MgSO 4 : (16.00) = g/mol Mg: 24.31/ x 100% = 20.20% Mg S: 32.06/ x 100% = 26.63% S O: 64.00/ x 100% = 53.17% O %H in C 2 H 5 O? Total mass C 2 H 5 O: 2(12.01) + 5(1.01) = g/mol C: 24.02/45.07x 100% = 53.29% C H: 5.05/45.07x 100% = 1.11% H O: 64.00/45.07x 100% = 35.50% O

8 22. Mole conversions (Ch 8): # of moles in 2.5g of Aluminum Oxide? 2.5 g x 1 mol =.025mol g # of moles in 15g of Neon? 15 g x 1 mol =.74mol 20.18g # of atoms in 0.5mol of Gold?.5 mol x 6.02 x atoms = 3 x atoms 1mol # of atoms in 1.5 grams of Zinc (II) Chloride? 1.5g x 1 mol x 6.02 x atoms = 6.6 x atoms g 1mol Chapter 9: Chemical Reactions and Equations Chemical reaction Reactant Product Chemical equation Coefficient Reaction Types Be able to Write and balance equations Identify types of reactions 23. Balancing equations (Ch 9): 4 Fe + 3 O 2 2 Fe 2 O 3 synthesis 3 Fe + 4 H 2 O 1 Fe 3 O H 2 single replacement 3 Mg + 1 N 2 1 Mg 3 N 2 synthesis

HONORS Chemistry Midterm Review

2015-2016 HONORS Chemistry Midterm Review This review sheet is a list of topics and sample practice problems only. The practice problems are good representation of what to expect on the midterm, but it