1 Practice Test Questions Chemistry Final Exam, May 24, 2016 Please note that this is not the format of the actual test. Answer the questions of this test to review your content knowledge. A. Atomic structure and chemical properties of elements If the statement is true, circle the letter T, if false circle F. 1. Atomic number represents the number of neutrons T F 2. An atom has a mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus. 3. A neutral atom of any element will contain the same number of protons and electrons. T T F F 4. An element always contains the same number of protons. T F 5. Isotopes are atoms of the same element with different numbers of neutrons T F Multiple Choice 6. Which of the following best describe the atomic mass? a) Number of protons b) Number of neutrons c) Number of protons and neutrons d) Number of protons and electrons 7. Which of the following best describe the atomic number? a) Number of protons b) Number of neutrons c) Number of protons and neutrons d) Number of protons and electrons 8. For the indicated element: 16 S 32.07 What is the atomic mass of this element? a) 8 AMU b) 16 AMU c) 32.07 AMU d) 48.07 AMU
2 Put the letter of the correct matches in the spaces to the left of each number. 1. Carry a positive electrical charge 2. Carry a negative electrical charge 3. Do not carry an electrical charge 4. Responsible for atomic mass 5. The basic substance that cannot be simplified 6. Atoms of elements chemically joined together a. Electron b. Proton c. Neutron d. Element e. Compound f. Protons and Neutrons B. Electron configuration 1. Carbon atomic number is 6. How many electrons does carbon have? A: 7 B: 12 C: 6 D: 8 2. Use the electron filling in the diagram to write the electron configuration for the following elements. 3. Atomic number of Neon is 10. Na atomic number is 11. Write the noble gas notation for the electron configuration of Na 4. Mg atomic number is 12, what is the noble gas electron notation of Mg? 5. How many valence electrons are there in Na? 6. How many valence electrons are there in Mg? 7. Atomic number of chlorine is 17. Write the electron configuration of chlorine. 8. How many valence electrons are there in chlorine 9. What is Octet rule
3 10. Use the Octet rule to determine the charge of the ions formed by the following atoms. Atom Na Al Cl Number of valence electron Oxidation number Ion C. The periodic table 1. Periodic table is an arrangement of elements in order of their a) atomic radius b) atomic mass c) atomic number d) chemical reactivity 2. The rows of the periodic table are called a) groups b) periods c) blocks d) trends 3. What is the most common charge of ions formed by the elements of the first column of periodic table? a) -1 b) -2 c) +1 d) 0 4. The atomic radii of elements in the periodic table a) increase across a row b) decrease across a row c) decrease down the column d) do not change down the column 5. Among the main-group elements, ionization energy a) decreases down the groups b) increases down the groups c) does not change down the groups d) decreases across a period 6. The size of an element s atomic radius _ from left to right across the periodic table. a. increases b. decreases c. remains constant d. is randomly assigned D. Chemical bonding - Ionic vs Covalent 1. A chemical bond results from the mutual attraction of the nuclei for a) electrons b) neutrons c) protons d) dipoles For questions 2-5, select the correct term to fill in the blank. 1. A _ bond is a bond where atoms share valence electrons. a) ionic b) metallic c) covalent 2. Covalent bonds always form between nonmetals and. a) metals b) nonmetals c) metalloids
4 3. An _ bond is a bond where electrons are transferred from one atom to another a) ionic b) metallic c) covalent 4. Ionic bonds always form between nonmetals and a) Metals b) Nonmetals c) Metalloids E. Writing chemical formula Write the chemical formulas for the following ionic compounds a) sodium Bromide b) aluminum bromide c) calcium carbonate d) aluminum sulfate F. Physical change vs chemical change Which one of the following is not a chemical change? a) Fall leaf color change b) Dissolving sugar in water c) Gasoline burning d) Milk turning sour G. Chemical reactions 1. The chemical reaction: 2 H2O 2 H2 + O2 a) synthesis reaction b) decomposition reaction c) single displacement reaction d) double displacement reaction e) combustion reaction 2. The chemical reaction: AgNO3 + NaCl AgCl + NaNO3 a) synthesis reaction b) decomposition reaction c) single displacement reaction d) double displacement reaction e) combustion reaction
5 3. The chemical reaction: AgNO3 + Cu Ag + CuNO3 a) synthesis reaction b) decomposition reaction c) single displacement reaction d) double displacement reaction e) combustion reaction 4. The chemical reaction: C3H8 + 5O2 3CO2 + 4H2O f) synthesis reaction g) decomposition reaction h) single displacement reaction i) double displacement reaction j) combustion reaction H. Write balanced chemical equations for chemical changes Balance the following chemical equations Al + Br2 AlBr3 CH 4 + O 2 _CO 2 + H 2 O I. Carbon compounds types of hydrocarbons 1. Hydrocarbons are; a. Compounds formed between water and carbon b. Molecules that contain only hydrogen and carbon c. A type of ionic compounds d. Organic molecules consisting of carbon, hydrogen and oxygen 2. Hydrocarbons that contain only single bonds are called a. Alkanes b. Alkenes c. Alkynes d. Alcohols 3. Hydrocarbons that contain double covalent bonds are called a. Alkanes b. Alkenes c. Alkynes d. Alcohols 4. Hydrocarbons that triple covalent bonds are called a. Alkanes b. Alkenes c. Alkynes d. Alcohols
6 5. An isomer is ; a. One of two or more compounds that have same chemical composition but different structures b. A type of hydrocarbon that have different structures resulting from differences in chemical composition c. One two closely related organic compounds d. An ionic compound Name the following chemical formulas ZnS Name: Name: Name: CaCl 2 MgCO 3 Name: Name: Name: J. Molecular weight and Mole calculations 1. In 1 mole of malic acid, C4H6O5, how many molecules are there? a. 6.02 x 10 23 molecules b. 7.53 x 10 23 molecules c. 1.27 x 10 27 molecules d. 1.78 x 10 22 molecules 2. Calculate the number of moles in each of the following a. 14.0 g of N b. 6g of C d. 64.1g of Al 3. Calculate the number of atoms in each of the following a. 14.0 g of N b. 6g of C d. 64.1g of Al 4. Calculate the mass of the following number of atoms a. 6.02 x 10 23 atoms of O b. 3.01x 10 23 atoms of C d. 1.50 x 10 23 atoms of Al