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Review Practice for Chemistry I Advanced freezing point _____ Measurements: 1. Identify as quantitative or qualitative data: red _______ three meters _______ 3. A student measures the volume of water to be 4.5 mL, 5.9 mL and 3.2 mL. If the water’s volume is actually 2.5 mL, how would you describe the student’s measurements in terms of accuracy and precision? How many significant digits does each of the following have: 45000 ____ 0.00320 ______ 5. Calculate the following using proper significant digits: 4.5 + 7.87 = ______ 6.53 x 2.345 _________ 6. What is the volume of a rectangle with the dimensions of 5.78 cm, 2.09 cm and 2.3 cm? ______ 7. Write the measurements in scientific notation: 789 000 km =______________ 0.00089 mm = _______________ What is the mass if the density is 1.87 g/cm3 and a volume of 4.5 cm3? What is the volume if the density is 0.76 g/ml and the mass is 6.7 grams? b. Why does an object sink? c. If a cube has one side measuring 2.0 cm3 and it has a mass of 30.0 g, what is its density? d. Aluminum has a density of 2.70 g/cm3 and iron has a density of 7.87 g/cm3. A substance has a mass of 45 g and a volume of 16.7 cm3, what is the substance likely to be? e. Look at the Y picture. The glass is filled with three different colorless liquids. Decide which letter represents the most dense object. How do you know? f. If a piece of wood with a density of 10.00 g/cm3 is cut in half, what is the density of each piece of wood? Why? Write the following in standard form: 5.6 x 10-2 cm ________________ 2.34 x 105 m = ______________ 9. What is the density of a substance with a mass of 16.5 grams and a volume of 3.6 mL? Round 54 6378 to three significant figures _________________ 4. 8. volume ____ 3. a. 2. odor _____ Do the following calculations to the correct number of significant digits. 5.6 x 102 X 2.34 x 105 = ________________ Be able to use dimensional analysis/factor label to make conversions. 56 g = _____________________ mg 2.6 days = _____________________ s 10. If you wanted to get the density of a block of wood, what tools would you need? 4. Identify as a physical and chemical change: Evaporation of alcohol ____ tarnishing silver ____ Leaves changing colors __ wood decays ____ Freezing water ___ biting a cookie ____ Combustion of oil ____ nail rusting _____ 5. Describe the difference between a mixture and a compound. If you wanted to get the density of a rock, what tools would you need? Matter and Change 1. Identify as a physical or chemical property Flammability ____ malleability ____ viscosity _____ 2. Identify as an intensive and extensive physical property. Red color ____ mass ____ density ____ X Give three examples of each. e. 6. A clear liquid evaporates and leaves a yellow solid. The original liquid was what type of matter? Explain. f. What is the mass number of the most common isotope of cobalt. _________ Write the nuclear notation for the most common isotope of chromium. 6. If a substance always has one atom of sulfur and three atoms of oxygen, it is an example of what type of matter? Explain. Identify the following as a pure substance (element or compound) or a mixture (homogeneous and heterogeneous). oxygen ___ dirt ____ sodium chloride ___ sugar water ___ muddy water ___ iron ____ 7. What is the smallest part of an element that has all of the properties of the element? __________ 8. Describe particles in the diagrams as being: mixtures, pure substances, compounds, and elements. Use the periodic table to find the following information concerning the element with 15 protons: a. Get the atomic number _________ b. Identify the element __________________ c. Find the mass number of the most common isotope of an element _________ d. Get how many neutrons the most common isotope has _________ e. How many valence electrons an element has _________ f. What is its charge/oxidation number for the atom _________ g. Know what ion is forms/write the ion _______ h. The name of the ion __________________ 7. Describe the three subatomic particles in the atom? Subatomic charge location particle 8. Atomic Structure: 1. 2. 3. 4. 5. What is the charge on the nucleus? ____________ What is inside the nucleus? ____________ What is the charge on the electron cloud? ____________ What is inside the electron cloud? ____________ Of the nucleus and the electron cloud, which is most dense? ____________ If an atom is electrically neutral, what is true about its particles? __________________________________________________ Define mass number. a. How is the mass number calculated? How do you find the number of neutrons an atom has? ______________________________________________________________ a. Define isotope: b. c. If two atoms are the same element, what must be the same? _______________________ The number written after the name of an isotope (Ex. Cabon-12), represents what? _________________________ d. 80Br 35 Identify the following: i. ii. iii. iv. Atomic number _________ Number of protons_________ Number of neutrons_________ Number of electrons _________ 9. Identify the protons, neutrons, and electrons b. What is this atom/element _____________ c. What is it’s mass number? _____________ There are four naturally occurring isotopes of the make-believe element Katrayden (Ka). Based on the following, what is the average atomic mass? 172 169 Ka 22.63 % Ka 6.42% 171 Ka 12.52% 170 Ka 58.43% Name an element in the same group as oxygen. ______ Electron Arrangement and Periodic Table: 1. Name the four sublevels and identify how many orbitals are in each. 11. Name an element with similar properties to magnesium. ______ How do you know? _________________ 2. How many electrons can occupy the s orbital? ____ p orbital? ____ How many electrons are needed to fill the 2nd energy level? ________ Identify this element: 1s2 2s2 How do you know? 12. Which has the smallest atomic radius: Mg or S Why? 3. 4. 5. Write the electron configuration for: Si 13. Repeat #12, but with which has the largest ionization energy. Mg or S Why/how do you know? Mg or Ca Why/how do you know? Ca Fe 6. Which has the smallest atomic radius: Mg or Ca Why? 14. Which element the largest electronegativity. ______ 15. How many valance electrons does each group 2A have?_______ group 6A? _____ Write the Aufbau diagram for: Li Bonding Cl 1. Identify the following as ionic or covalent: a. HCl ____ d. NO _____ b. MgCl2 ____ e. CCl4 ____ c. SF2 ____ f. Na3P ____ 2. How many bonds do each of the following tend to form? C ___ O ____ N ___ H_____ 3. List four properties of covalent compounds: 4. List four properties of ionic compounds: 5. List the seven diatomic molecules and indicate the number of bonds between them. 6. Draw the following Lewis structures and identify their shape. CF4 CO2 Mg 7. Write the noble gas notation for: S K Fe 8. How many electrons are in the highest energy level of: 1s2 2s22p6 3s2 3p64s23d2 _____ Identify this element ___________________ 9. Describe each of the following in terms of valence electrons, block on periodic table, and outer electron configuration: alkali family, alkaline-earth metals, halogens and the noble gases by completing the table: Alkali Alkalineearth halogens H2O NH3 PH3 CBr3F Noble gases Valence electrons Block on periodic table Outer electron configuration 10. Name an element in the same period as lithium. ______ Mole …is back 1. How many atoms are in 1 mol iron? ________________ Lithium? ________________ 2. What is the molar mass of manganese? ________ Oxygen? ________ Gold? ________ 3. How many moles of magnesium are in 35.6 g of magnesium? How many moles of lithium are in 75.89 g of lithium? How many atoms are in 6.53 moles of carbon? How many atoms are in 13.8 moles of Chromium? Identify the following pieces of lab equipment and what they are used for.