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Chemistry Fall Semester Exam Review 2013

Chemistry Fall Semester Exam Review 2013 . Ms. Johnson  10 th Grade Chemistry. 1). Describe the differences between solids, liquids, and gases. Draw a diagram of atoms in the solid state changing to liquid state changing to gaseous state.

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Chemistry Fall Semester Exam Review 2013

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  1. Chemistry Fall Semester ExamReview 2013 Ms. Johnson  10th Grade Chemistry

  2. 1). Describe the differences between solids, liquids, and gases. Draw a diagram of atoms in the solid state changing to liquid state changing to gaseous state. • Solidshave tightly packed particles, with high density. They have a definite volume and shape. • Liquids have particles that move past each other. Their density is lower than solids. They have definite volume but take the shape of their container. • Gases have particles that are very far apart from each other. They have a density about 1000 times less than a solid. They take the volume and shape of whatever container they are put in.

  3. 2).Explain the difference between an extensive property and an intensive property. Give 4 examples of each. • Extensive properties depend on the amount of matter that you have: mass, volume, length, amount of energy. • Intensive properties do not depend on the amount of matter present: density, boiling point, melting point, ability to conduct heat/electricity.

  4. 3). Explain the difference between a physical change and a chemical change. Give 4 examples of each. • Physical changes do not change the identity of the substance: cutting paper, dissolving a solid in water, boiling, freezing. • Chemical changes result in a new substance being formed: burning charcoal, digesting food, photosynthesis, forming water from hydrogen and oxygen.

  5. 4).Explain the difference between a mixture and a pure substance. Give 4 examples of each. • A mixture is a blend of substances that can be physically separated: oil and water; salt and sand; blood; milk. • A substance is a form of matter that cannot be broken down without a chemical reaction—it is either an element or a compound: CO2, H2O, copper, gold

  6. 5). Explain what apparatus and procedure you would use to separate a mixture of sand, salt, water, and iron shavings. • 1).Use a magnet to separate the iron from the mixture. • 2).Add the sand and salt mixture to water to dissolve the salt. • 3).Pour the mixture through a filter to separate out the sand. • 4).Boil the saltwater solution to remove the water and remain with salt.

  7. 6). For each scientist in the table below, discuss their experiment, including special equipment, their key conclusion, and how it changed our view of the atom:

  8. 7). Using the table above, find the atomic mass of the element. • Average atomic mass = (.6917 x 62.929) + (.3083 x 64.927) = 63.54 amu

  9. 8). Solve the following mole calculations: • a. How many grams are in 4.23 moles of calcium? • 4.23 molCa x = 170 g Ca • b. How many moles are in 56.98 grams aluminum? • 56.98 g Al x = 2.112 mol Al • c. How many atoms are in 13.5 grams of zinc? • 13.5 g Zn x x = 1.24 x 1023 atoms Zn • d. How many moles are in 3.450 x1023 atoms of lead? • 3.450 x1023 atoms of Pb x = 0 .5731 molPb

  10. 9).Perform the following calculations • a. Find the density of a rock with mass of 14.5 g and volume of 2.35 mL. • d = = = 6.17 g/mL • b. Find the volume of a substance with density of 1.79 g/mL and mass of 34.5 g. • v = = = 19.3 mL • c. Find the mass of a coin with volume of .75 cm3 and density of 2.73 g/cm3. • m = d·v = (.75 cm3)(2.73 g/cm3) = 2.05 g

  11. 9).Perform the following calculations • d. 12.5 m to cm = • 1250 cm • e. 8.7 g to kg = • 0.0087 kg • f. 42.0 mL to nL = • 4.2 x 107nL

  12. 10). Determine the number of significant figures in the following measurements • a. 20.00 _________ • 4 • b. 184,345 ________ • 6 • c. 40.080 ________ • 5 • d. 4,000,000 _______ • 1

  13. 11). Define the mole • The mole is a number. There are three equation for mole conversions: • Def. of Mole Equation: 1mol = 6.02 x 1023atoms, molecules, particles • Molar Mass Equation: 1mol = _________ grams • Volume at STP: 1 mol = 22.4 L • a. How many atoms are in 1 mole of zinc? • 6.02 x 1023 atoms of Zn • b. How many grams are in 1 mole of zinc? • 65.38 g/mole of Zn

  14. 12). Sketch out the electromagnetic spectrum. Include: x-rays, microwaves, gamma rays, UV light, IR light, visible light, and radio waves. • a. Show how the frequency of electromagnetic radiation goes from low to high across the spectrum. • b. Show how the wavelength of electromagnetic radiation goes from long to short across the spectrum. • c. Show how the energy of electromagnetic radiation goes from low to high across the spectrum. low frequency high frequency long wavelengthshort wavelength low energy high energy • Radio,TV microwaves,radarIRvisible lightUVX raysGamma rays

  15. 13).Sketch out the visible light spectrum. Label the colors. • a. Show how the frequency of electromagnetic radiation goes from low to high across the spectrum. • b. Label 400nm and 700nm. • c. Show how the energy of electromagnetic radiation goes from low to high across the spectrum. • low frequency high frequency • 700 nm wavelength R O Y G B I V400 nm wavelength • low energy high energy

  16. 14). Perform the following calculations: • a. What is the frequency of electromagnetic radiation with a wavelength of 1.5 x 10-3 m? • frequency = speed of lightwavelength(f=c/λ ) • = = 2.0 x 1011Hz • b. What is the wavelength of electromagnetic radiation with a frequency of 2.8 x 1015 Hz? • wavelength = speed of lightfrequency(λ = c/f) • = = 1.1 x 10-7 m • c. What is the energy of electromagnetic radiation with a frequency of 5.9 x 1016 Hz? • energy = Planck's constant x frequency (E=hf) • = (6.63 x 10-34 Js)(5.9 x 1016 Hz) = 3.91 x 10-17 J

  17. 15). Write the electron configuration and noble gas configuration for the following elements: • Phosphorus (atomic #15) • 1s22s22p63s23p3 & [Ne] 3s23p3 • Palladium (atomic #46) • 1s22s22p63s23p64s23d104p65s24d8 & [Kr] 5s24d8 • Potassium (atomic #19) • 1s22s22p63s23p64s1 & [Ar] 4s1

  18. 16).For each of the following groups, what ending electron configuration do the elements have? • a.Group1 and 2 elements • Group 1: s1 Group 2: s2 • Group 13 to 18 elements • all end with p, from p1 (group 13) to p6 (group 18) • transition metals • all end with d, from d1 to d10 • inner transition metals • all end with f, from f1 to f14

  19. 17).Explain the contributions of Mendeleev and Mosely to the modern periodic table arrangement. • Dmitri Mendeleev gets credit as "Father of the Periodic Table." He arranged the elements by mass and reactivity, leaving blank spaces for those he thought were still undiscovered. • Moseley later rearranged the table by atomic number.

  20. 18).For each of the following families on the periodic table, list how many valence electrons they have and what you know of their properties:

  21. 19). Explain the group and period trends on the periodic table for the following a). atomic radius: • group trend--radius increases, because additional energy levels are further from the nucleus • period trend--radius decreases, because electrons are added at the same energy level and are increasingly attracted to the larger nucleus b). ionization energy: • group trend--energy decreases, because it is easier to remove electrons that are further from the nucleus • period trend--increases, because it is more difficult to remove the electrons as they are increasingly attracted to the larger nucleus c). electronegativity: • group trend--in general, decreases down a group • period trend--in general, increases across a period • Highest electronegativity: fluorine • Lowest electronegativity: cesium.

  22. 20).Fill out the table below for the different types of bonds:

  23. 21).Explain how electrons move in a metallic bond and why they are considered good conductors of heat and electricity, malleable, and ductile. • Metal atoms pack closely together and their outer orbitals overlap. This allows the valence electrons to move freely throughout the lattice. These are known as delocalized electrons. The attraction between the metal cations and the surrounding sea of valence electrons is known as metallic bonding. • The free movement of the valence electrons is what allows for electrical conductivity--the electrons move towards a positive charge, and this movement is a current. Because there are no repulsive forces within a metal lattice, any force on the lattice causes its structure to rearrange, rather than break, which accounts for the malleability and ductility of metals.

  24. 22).Draw the Lewis dot structure for the following ionic compounds • a. K3P • b. CaCl2

  25. 23).Draw the Lewis dot structure for the following compounds and identify the molecular and electron pair geometries of each • a. CH4 • Tetrahedral • b. H2O • Bent

  26. c. NH3 • trigonal pyramidal • d. CO2 • linear • e. BH3 • Trigonal planar

  27. 24). Write the chemical formula for each of the following: • a. lead (II) oxide PbO • b. lead (IV) sulfide PbS2 • c. barium nitrate Ba(NO3)2 • d. aluminum hydroxide Al(OH)3 • e. zinc chloride ZnCl2 • f. copper (II) oxide CuO • g. potassium sulfate K2SO4 • h. potassium oxide K2O • i. cobalt (III) fluoride CoF3 • j. copper(II) sulfate pentahydrateCuSO4. 5H2O

  28. 25).Name the following compounds: • a. PBr5phosphorous pentabromide • b. PbI4lead (IV) iodide • c. N2O3dinitrogentrioxide • d. SO3sulfur trioxide • e. Ag3PO4silver phosphate • f. CaOcalcium oxide • g. Cu(OH)2copper (II) hydroxide • h. CoCl2·6H2Ocobalt(II) chloride hexahydrate • i. HClhydrochloric acid • j. NH4Brammonium bromide

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