Chemistry Semester 1 Final Review

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elevation 5) What is the dependent variable? temperature 6) What is the temperature at an elevation of 400 m? 17.5 C 7) What technique did you use to answer question 6? interpolation (est.

1 NAME: Chemistry Semester 1 Final Review 1) What type of graph is this? Pie/circle 2) What percent of chlorine in the stratosphere is a natural source? 18% 3) How many different sources of chlorine in the stratosphere are there? 8 Use the chart below to answer questions ) What is the independent variable? elevation 5) What is the dependent variable? temperature 6) What is the temperature at an elevation of 400 m? 17.5 C 7) What technique did you use to answer question 6? interpolation (est. within data) 8) Is the slope positive or negative? How can you tell? negative; y/ x = negative 9) Fill in the chart with the appropriate SI units and symbols. pg. 63 Quantity SI Unit Symbol Length meter m Mass kilogram kg Time second sec or s Temperature Kelvin K 10) Convert the following measurements. a. 75 m = 7500_ cm c kg = 350 g b. 9.3 ml = 0.093_ dl d kl = 6_ L 11) Write the equations for converting Kelvin to Celsius and Celsius to Kelvin. a. K = C b. C = K c. If a liquid freezes at 26 C, what is its freezing point in Kelvin? K = 26 C = 299K

12) Label the charts below as either accurate, precise, both, or neither. (Only 1 arrow!) accurate precise both neither 13) Differentiate between qualitative and quantitative data.

Theory: thoroughly tested model which explains experimental results c. Control: standard for comparison d. Independent Variable: variable being manipulated (changed) in an experiment e.

2 12) Label the charts below as either accurate, precise, both, or neither. (Only 1 arrow!) accurate precise both neither 13) Differentiate between qualitative and quantitative data. Qualitative = descriptive, non numeric Quantitative = numerical 14) Define the following steps of the scientific method: a. Hypothesis: proposed explanation for observations b. Theory: thoroughly tested model which explains experimental results c. Control: standard for comparison d. Independent Variable: variable being manipulated (changed) in an experiment e. Dependent Variable: variable being observed after manipulation (changing) of the independent variable 15) What is the density of aluminum if a 55.5 g sample occupies 21.0 cm 3? D = M/V = 55.5g/21.0cm 3 = 2.64 g/cm 3 (make sure your sig figs are correct) 16) If aluminum s actual density is 2.70 g/cm 3, what is the percent error in the measurement above? (from questions 15) 17) How many significant figures are in the following numbers? a c b x10-9 d. unlimited 1 mole = 6.02 x atoms 18) Convert to scientific notation x ) Convert 8.73 x 10-3 to standard notation ) Calculate the following problems. Use correct sig figs! a. (2.32 x 10 5 cm) + (3.5 x 10 3 cm) = 2.36 x 10 5 cm b. (5.400 x 10 3 m) x (3.13 x 10 4 m) = 1.69 x 10 8 m 2 c. (8.444 x 10-4 m 3 ) / ( x 10-3 m 2 ) = x 10-2 m 21) How many cm are in 12.5 m?

3 22) How many km are in 3.85 dm? 23) If a car is traveling at 9.8 m/s, how many hours will it take to travel 170 km? 24) If the density of a substance is 15.2 g/ml, what is its density in cg/kl? 25) Define the following terms and give an example of each. a. Chemical property ability to undergo a chemical reaction and form new substances. Ex. flammability, reactivity b. Physical property quality of a substance which can be observed or measured without changing the substance s chemical composition. Ex. melting point, boiling point, color, solubility, hardness, density c. Chemical change altering a material with changing its chemical composition. Ex. burning, reacting, rusting, corroding, d. Physical change altering a material without changing its chemical composition. Ex. hammering, melting, boiling, cutting, e. Intensive Property independent of the amount of substance present ex. density, color f. Extensive Property dependent upon the amount of substance present ex. mass, length, volume 26) Koolaid is an example of a homogeneous mixture whereas Italian salad dressing is an example of a heterogeneous mixture. 27) Fill in the following chart. (definite or indefinite) State of Matter Shape Volume Solid Definite definite Liquid Indefinite definite Gas Indefinite indefinite 28) A 24-g sample of carbon combines with 64 g of oxygen to form CO 2. a. What is the mass of the reactants? 24 g + 64 g = 88 g b. What is the mass of the product? 24 g + 64 g = 88 g c. Which law do these data support? Law of Conservation of Mass 29) A g sample of milk of magnesia,, always contains g of magnesium, g of oxygen, and 2.02 g of hydrogen. Find the mass percentage of each element in milk of magnesia. Total mass = 24.31g g g = 58.33g a. Mg (magnesium) = (24.31/58.33)*100 = 41.68% b. O (oxygen) = (32.00/58.33)*100 = 54.86% c. H (hydrogen) = (2.02/58.33)*100 = 3.46% 30) Fill in the following chart Isotope Symbolic Mass Number of Number of Number of

4 Notation Notation Number Protons Neutrons Electrons Hydrogen Oxygen Copper Uranium ) How are isotopes of the same element different? How are they the same? Different = number of neutrons, mass number Same = number of protons, electrons 32) Antimony (Sb) has two stable isotopes. Anitmony-121 has an abundance of 33.0% and Antimony-123 has an abundance of 67.0%. What is antimony s average atomic mass? 33) Label the type of reaction and fill in the missing particle C Type:_Beta decay Type:_Alpha _ Type:_Beta 14 7 N 0-1 e 34) Define the following terms: a. frequency number of wave cycles that pass a given point per unit of time b. wavelength distance between two adjacent crests of a wave c. quanta (plural of quantum) amount of energy needed to move an electron from its present energy level to the next higher one. d. orbital region around the nucleus where there is a 90% chance of finding an electron. 35) Arrange the following electromagnetic radiation in order of increasing energy and frequency. Ultraviolet light, x-ray, micro waves, red light, infrared ) Fill in the following table. Principal Quantum Number, n Th 88Ra Ra 1e Types of Orbitals Number of Orbitals Related to Principal Energy Level 1 s 1 2 s & p 4 3 s, p, & d 9 4 s, p, d, & f 16 37) How many electrons are in: a. the first energy level? _2 He Ac

5 b. the 3d sublevel? 10 c. 4th principal energy level? 32 d. the 3f sublevel? none e. the 3p sublevel of sulfur? 4 38) Write the orbital (arrows!) notation for nitrogen. 1s 2 2s 2 2p 3 (epic failure!) 39) Write the electron configuration for copper. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 40) Write the electron configuration, noble gas configuration, and electron dot for the following elements. a. Ca = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 or [Ar]4s 2 (2 valance electrons) b. Ar = 1s 2 2s 2 2p 6 3s 2 3p 6 or [Ne]3s 2 3p 6 (8 valance electrons) 41) Identify each atom. a. 1s 2 2s 2 2p 1 (boron) b. [Ar]4s 1 (potassium) 42) What is the energy of a photon of electromagnetic radiation being emitted by a radio station broadcasting at a frequency of x 10 2 MHz? 43) What is the frequency of infrared light with a wavelength of 1200 nm? 44) What is the wavelength of x-ray radiation with energy of 3.1 x 10-8 J? Two ways to solve: 1) use both E = hv & c = λv or 2) combine equations to get: 45) Briefly describe the contribution of each of the following to the development of the periodic table. a. Henry Moseley: organized by atomic number b. Dmitri Mendeleev: organized by atomic mass and similar chemical properties Match each of the following terms with a number or chemical symbol from the periodic table below. 46) alkali metals (1) 47) alkaline earth metals (2) 48) d-block element (Ni) 49) f-block element (Th)

6 50) halogens (4) 51) inner transition metals (6) 52) metalloid (Si) 53) noble gases (5) 54) a p-block element that is not a metalloid (O) 55) an s-block element (Be) 56) transition metals (3) 57) What groups are the representative elements? 1A through 8A 58) Define the following: a. Group: column on period table b. Period: row on periodic table c. Atomic Radii: distance between the two nuclei of adjacent atoms d. Ionization Energy: energy required to remove an electron from an atom e. Electronegativity: tendency for an atom to attract electrons to itself when it is chemically combined with another element 59) What is the trend for each of the following (down a group and across a period): a. Atomic Radii increases down a group; decreases across a period b. Ionization Energy decreases down a group; increases across a period c. Electronegativity decreases down a group; increases across a period 60) Which is bigger, Sr or Sr +2? Sr 61) non-metals generally form anions. (negative charge) 62) metals generally form cations. (positive charge) 63) What particle determines most of the properties of elements? electrons 64) Write the formulas of the following compounds. a) chlorine triiodide ClI 3 d) dinitrogen tetroxide N 2 O 4 b) cobalt (II) phosphate Co 3 (PO4) 2 e) sodium sulfate Na 2 SO 4 c) barium oxide BaO f) titanium (IV) sulfide TiS 2 65) Name the following compounds. a) LiCl Lithium chloride d) Fe(NO 3 ) 3 Iron (III)nitrate b) F 2 Fluorine e) N 2 O 5 dinitrogen pentoxide c) CaCl 2 Calcium chloride f) CO 2 carbon dioxide 66) Why do elements form bonds? to become stable by obtaining 8 valance electrons

7 67) What happens to electrons in an ionic bond? bond, ionic bond, taken not shared 68) What happens to electrons in a metallic bond? delocalized electrons, electron sea 69) What happens to electrons in a covalent bond? Shared 70) Determine the bond type for the following elements. Use page 405 for electronegativity values. a. Na & F - ionic b. C & O polar covalent c. H & Br polar covalent 71) Define the following terms. a. Resonance one Lewis structure does not correctly represent the structure of the molecule. b. Octet rule Atoms gain, lose or share electrons to obtain 8 electrons c. VSEPR Valance Shell Electron Pair Repulsion electrons repel each other and form arrangements which will minimize the repulsions. 72) Draw the Lewis structure, shape, hybridization, bond type, molecule type, and the intermolecular force for each of the following substances. a. H 2 S bent, sp 3, NPC, P, dipole-dipole b. NCl 3 - tri. Pyramid, sp 3, NP, P, dipole dipole c. CB r4 tetr., s p3, PC, nonpolar, LDF d. SO 3 tri. Planar, sp 2, PC, non-polar molecule, LDF 73) How many sigma and pi bonds are in each substance from #72? # sigma #pi a. 2 0 b. 3 0 c. 4 0 d ) Predict the products and balance each reaction. a. 2Na + Cl 2 2NaCl b. 2BF 3 2B + 3F 2 c. Al + 3CuNO 3 Al(NO 3 ) 3 + 3Cu d. C 5 H O 2 5CO 2 + 6H 2 O

8 75) Write the complete ionic and net ionic equation of Ca(NO 3 ) 2(aq) + Na 2 SO 4(aq) CaSO 4(s) + 2NaNO 3 Complete Ionic Equation: Ca 2+ (aq) + 2NO 3 - (aq) + 2Na + (aq) + SO 4 2- (aq) CaSO 4(s) + 2Na + (aq) + 2NO 3 - (aq) Net Ionic Equation: Ca 2+ (aq) + SO 4 2- (aq) CaSO 4(s)

Solid Gas Liquid Plasma

Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and