SCI-CH Remediation C 2 Exam not valid for Paper Pencil Test Sessions

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1 SCI-CH Remediation C 2 Exam not valid for Paper Pencil Test Sessions [Exam ID:0WFDJP 1 Which scientist speculated that atoms of the same element are identical to one another? A Dalton B Bohr C Thompson D Rutherford 2 Where is a neutron located? A Cytoplasm B Outside Nucleus C Mitochondria D Nucleus 3 The atomic number of silver-108 is A 108 B 47 C 107 D 61 4 Compared to the radius of a calcium atom, the radius of a calcium ion is A larger because it has lost two electrons B smaller because it has gained two electrons C larger because it has gained two electrons D smaller because it has lost two electrons

2 5 An atom has an electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1. The oxidation number of this atom would be A 2 + B 1 + C 1 - D 2-6 An atom, which is an isotope of an element, is characterized by A having more protons in its nucleus B having more electrons in its nucleus C having fewer protons in its nucleus D having more neutrons in its nucleus 7 Atoms gradually get smaller moving across a row on the periodic table because A they have more electrons B the central charge is larger and pulls electrons closer to the nucleus C atoms lose an energy level moving across a period D they have fewer protons 8 What is the mass of a proton? A x B x C x D x Which periodic trend decreases across a period but increases down a group? A Ionization energy B Electronegativity C Electron affinity D Atomic radius

3 10 When the products of a reaction have different chemical and physical properties than the reactants that formed them, it is an indication that A a chemical change has occurred B the reactants have exceeded their shelf-life C a physical change has occurred D no change has occurred 11 Vertical columns on the periodic table have predictable properties because of their A increasing atomic radius B decreasing electron affinity C similar valence electron configurations D decreasing electronegativity 12 In Rutherford s gold foil experiment, he concluded that the atom is mostly made-up of A empty space B electrons C neutrons D nucleus 13 Lithium, sodium, potassium, rubidium, cesium, and francium belong to the A alkali metals B halogens C transition metals D alkaline earth metals 14 All of the following are associated with Bohr s model EXCEPT A atoms have definite orbits for electrons B electrons can change energy levels C energy levels farthest from the nucleus have higher potential energy D energy levels closest to the nucleus are higher in energy

4 15 Chromium-50, chromium-52, chromium-53, and chromium-54 are all natural occurring isotopes of chromium. The isotopes of chromium differ in their A number of protons B atomic mass C atomic number D electron configuration 16 Which theory states that energy is absorbed or radiated in discrete units? A Relativity B Heisenberg uncertainty principle C Quantum D Conservation of energy 17 A measure of the ability of an atom in a chemical compound to attract electrons is called A atomic radius B ionization energy C atomic number D electronegativity 18 What is a chemical property of water? A It contains a regular crystalline structure in its solid form. B It boils at 100 C at 1 atm of pressure. C It freezes at 0 C at 1 atm of pressure. D It decomposes into H 2 and O 2 gas. 19 When a strontium atom loses its valence electrons, it has the same electron configuration as which element? A Rb B Ar C Kr D Xe

5 20 The subatomic particle(s) responsible for giving an element its identity is the A proton B atomic mass C neutron D electron 21 Nuclear chemistry deals with the nuclei of atoms breaking apart. When this occurs radioactive particles alpha, beta, and gamma are released. Which of these radiation types has the greatest penetrating power? A Beta B Alpha C Gamma D Radioactive particles 22 Millikan s oil drop experiment led to the discovery of A the size of a proton B the overall charge of an atom C the electrical charge of an electron D the electrical charge of a proton 23 In the experiment with cathode ray tubes, J.J. Thomson concluded that the cathode rays were composed of particles that were A positively charged B negatively charged C visible D neutral 24 For the elements Rb, F, and O, which lists these elements in order of increasing electronegativity? A Rb < F < O B Rb < O < F C O < F < Rb D F < O < Rb

6 25 What is the symbol for the ion that has 7 protons and 10 electrons? A Al 3+ B N 3- C B 3+ D P 3-26 How many protons are in the calcium ion, Ca 2+? A 20 B 18 C 40 D 2 27 What lists the elements Kr, C, Br and Se in order of increasing atomic size? A C < Kr < Br < Se B Kr < Br < Se < C C Br < C < Kr < Se D Se < Br < Kr < C 28 A halogen will readily react with A an alkaline earth metal B another halogen C a noble gas D an alkali metal 29 The density of a substance that has a mass of 7.0 g and a volume of 3.4 cm 3 is A 3.4 g/cm 3 B 24 g/cm 3 C 7.0 g/cm 3 D 2.1 g/cm 3 30 The concept that the location and velocity of an electron cannot be know simultaneously is A aufabau principle B quantum principle C Pauli exclusion principle D Heisenberg uncertainty principle

7 31 The element in group 14, period 2 is abundantly found in A sand, quartz, rock crystals, flint, and opals B stellar energy production, the human body, and water C food, fertilizers, ocean water, and explosives D stars, the Sun, comets, and the Earth's atmosphere 32 The graph represents the decay of a radioactive isotope. What is the half-life of this isotope? A 40 hours B 80 hours C 55 hours D 11 hours 33 The atomic number of an element includes A the number of electrons plus the number of neutrons B the number of protons plus the number of electrons C the number of protons in the nucleus D the number of protons plus the number of electrons and neutrons 34 All of the following have the same number of valence electrons EXCEPT A Se 2- B [Ar]3s 2 3p 6 C Ge D As 3-

8 35 A factor that tends to lower ionization energy within a family as atomic number increases would be A increased shielding effect from the inner electrons B decreased shielding effect from the inner electrons C increased electronegativity D decreased electronegativity 36 What scientist explained the theory of atomic structure by relating it to the planetary model? A Dalton B Bohr C Lavoisier D Thomson 37 Which statement is included in Dalton s Atomic Theory? A Atoms of different elements combine in whole number ratios to form compounds. B Atoms cannot be separated, combined or rearranged in chemical reactions. C Atoms can be created and destroyed in chemical reactions. D All atoms of a particular element are not identical. 38 Which element is found in Period 2 and Group 13? A Boron B Nitrogen C Carbon D Beryllium 39 Noble gases are chemically inactive because A they do not have valence electrons B their outermost energy level is filled and stable C they cannot add or lose protons D their atomic structure can vary depending on reaction type 40 Which law states that when elements are arranged in order of increasing atomic numbers, their physical and chemical properties show a periodic pattern? A Periodic law B Law of octaves C Law of conservation of matter D Law of reactiveness

9 41 The halogen family (group 17) shares which main characteristics? A Electron affinity B Atomic radius C Boiling point D Chemical properties 42 The periodic law states that periodic repeating patterns in physical and chemical properties are observed when elements are arranged according to their A increasing atomic size B period number C alphabetically grouped symbols D increasing atomic numbers 43 Which scientist was given the distinction as the Father of Modern Chemistry? A Mendeleev B Proust C Lavoisier D Dalton 44 Horizontal rows on the periodic table have predictable properties because of the A increasing numbers of neutrons across the period B decreasing numbers of neutrons across the period C increasing numbers of electrons across the period D decreasing numbers of electrons across the period 45 An atom has an electron configuration of 1s 2 2s 2 2p 5. The element belongs to the A noble gases B alkali metals C carbon family D halogens

10 46 Which of the following will NOT be decomposed by a chemical change? A KCl B H 2 O C CO D Co 47 Removing an electron from an atom with an electron configuration of 1s 2 2s 2 2p 6 3s 1 would A produce an anion B produce a cation C change the identity of the atom D change the atomic mass of the atom 48 In the diagram, what is represented by the outer region of the atom? A Electromagnetic radiation B Radioactivity C An electron cloud D A mushroom cloud 49 The elements that are located in Groups 3-12 of the periodic table are known as the A alkali metals B alkaline earth metals C metalloids D transition metals

11 50 The average atomic mass of an element is determined by its A most abundant isotope B radioactive isotopes C artificial isotopes D naturally occurring isotopes 51 On the periodic table, the element with the smallest electronegativity is A lithium B fluorine C oxygen D francium 52 Which diagram below depicts the atom with the lowest first ionization energy? A B C D 53 Which model is used to show the paths of electrons in an atom? A Ball and stick model B Bohr s planetary model C Dalton's model D Thomson s plum-pudding model 54 What particle has a negative charge and is approximately 1/2000th the mass of a proton? A anti-proton B alpha particle C neutron D electron

12 55 An element s average atomic mass is dependent on the masses of its isotopes and each isotope s A relative abundance B mass number C atomic number D number of neutrons in the element 56 Indium-115 has a half-life of 4.5 hours. A 24.0 mg sample of indium under goes radioactive decay. How much indium would remain after 27 hours? A 5.33 mg B 24.0 mg C 12.0 mg D.375 mg 57 Which refers to the state of an electron in its lowest energy level? A Energy B Excited C Ground state D Normal 58 Fluorine, F, shares similar chemical and physical properties with A oxygen, O B neon, Ne C chlorine, Cl D argon, Ar 59 Isotopes of the same element must have the same A atomic number B number of neutrons C number of electrons D mass number 60 Which example is NOT a compound? A B PO CO C NH 4 D Pb

13 61 All atoms of the same element have the same number of A nucleons B protons C electrons D neutrons 62 How many valence electrons are present in a neutral atom of sulfur? A 2 B 4 C 8 D 6 63 Which represents an atom of magnesium? A 3 B 4 C 2 D 1 64 The half-life of a radioisotope is 30 days. What will remain of a 20.0 g sample after 90 days? A 2.5 g B 17.5 g C 1.25 g D 10 g

14 65 Carbon-14 is used in radioactive dating to determine the age of fossils. Carbon-14 is an A atom B ion C isotope D element 66 Moving across a period on the periodic table, each element gains one A proton B nucleus C oxidation number D neutron 67 An ion that possesses 12 protons and 10 electrons is A Mg 2+ B 0 2- C F 1- D Al Neutral atoms A have the same number of protons as electrons B always have isotopes C have the same number of electrons as neutrons D have the same number of protons as neutrons 69 The following are characteristics of metals with the exception of A conductors of electricity B malleable C ductile D low melting point

15 70 The transition elements are characterized by having an incomplete A p sublevel B f sublevel C d sublevel D s sublevel 71 When moving across a period or down a group, the atomic mass increases. This trend can be explained by the A electrons increasing in mass as the atomic mass of the atom increases B protons increasing in mass as the atomic mass of the atom increases C addition of electrons to the atomic nucleus D addition of protons to the atomic nucleus 72 The following entry for potassium was taken from the periodic table of elements. A neutral atom of potassium has A 19 protons, 20 neutrons, 20 electrons B 19 protons, 19 neutrons, 19 electrons C 19 protons, 20 neutrons, 19 electrons D 20 protons, 19 neutrons, 20 electrons 73 Ductility and malleability are examples of A physical properties B properties of nonmetals C chemical properties D reactive properties 74 What is the atomic number of a member of the halogens? A 18 B 17 C 10 D 8

16 75 Experimental data shows that the nucleus of an atom A contains mostly negative charge B contains most of the mass of the atoms C has no charge D is mostly empty space 76 Identify the element located in period 3, group 14. A Silicon, Si B Scandium, Sc C Carbon, C D Phosphorus, P 77 Which example would be classified as heterogeneous matter? A A solution B An element C A compound D A mixture 78 What is the name of the third major subatomic particle, labeled number 1, in the shown chart? A Electron B Nucleus C Cathode D Electrode 79 Elements in the same family on the periodic table have the same A atomic mass B number of valence electrons C number of neutrons D atomic number

17 80 Which two particles have approximately the same mass? A electron and neutron B neutron and alpha particle C proton and electron D proton and neutron 81 All atoms on the periodic table will gain or lose electrons in order to gain an electron configuration similar to a A transition element B halogen C metal D noble gas 82 Silicon-28, silicon-29, and silicon-30 are three naturally occurring isotopes of silicon. The fractional abundance of these isotopes in nature is 92.21%, 4.70%, and 3.09%, respectively. The proper mathematical calculation for the average atomic mass of silicon is A [( )] + [( )] + [( )] B [(28)(.9221)] + [(29)(.0470)] + [(30)(.0309)] C [( )] + ( )] + [( )] D [( )] [( )] [( )] 83 Which nucleus is an isotope of the figure shown? A B C D 84 The modern periodic table is arranged according to A alphabetical order B reactivity C atomic number D atomic mass

18 85 Each period of the periodic table ends with a A alkali metal B metalloid C noble gas D halogen 86 Which properties describe the Group 1 Alkali Metals? A Not highly reactive and tend to form unstable compounds. B Not highly reactive and tend to form stable compounds C Highly reactive and tend to form stable compounds D Highly reactive and tend to form unstable compounds 87 What is one indication that an electron has dropped from a higher to a lower energy level? A The emission of light B The decrease in size of the atom C The absorption of light D The increase in size of the atom 88 Which law states that the properties of elements repeat every eight elements? A Law of conservation of matter B Law of octaves C Law of reactiveness D Periodic law 89 Which of the following is the best conductor of electricity? A NaCl(s) B NaCl(aq) C CH3COOH(s) D CH3COOH(aq)

19 90 What should replace the number 2 in the shown chart? A +2 B -1 C +1 D 0 91 With n representing the outermost energy level, ns 2 np 2 represents the electron configuration for an element in A Group 12 B Group 4 C Group 2 D Group Which scientist is attributed with developing the modern periodic table of elements by atomic mass? A Lavoisier B Mosley C Democritus D Mendeleev 93 The atomic number of an element is always equal to the number of A protons B neutrons C protons plus neutrons D protons plus electrons 94 In the reaction, uranium-238 loses two neutrons and two protons to form thorium-234. This is an example of A an alpha decay B a radioactive dating decay C a beta decay D a gamma decay

20 95 Which nuclear particle has the greatest mass? A electron B beta particle C neutron D alpha particle 96 A chloride ion, Cl 1- contains A 17 electrons B 15 electrons C 18 electrons D 16 electrons 97 The above experiment was created and used by which scientist? A Robert Millikan B Neils Bohr C John Dalton D Joseph Thomson

21 98 Using the graph, what general trend exists for the first ionization energy within a period? A Ionization energy decreases B Ionization energy increases C Ionization energy increases then decreases D Ionization energy remains constant 99 Which of the following orbital diagrams is incorrect because it violates Hund s rule? A B C D 100 The atomic number corresponds to an atom s number of A protons B neutrons C positrons D electrons

22 101 Which of the following properties decreases from left to right across a period? A Ionization energy B Atomic radius C Electronegativity D Atomic number 102 The figure above shows a compound containing hydrogen (H) and an unknown element Z. To which group on the periodic table does element Z belong? A 14 B 16 C 15 D Which of the above elements is a positive ion with a charge of one? A 4 B 2 C 1 D Cations are formed when neutral atoms lose A positrons B protons C neutrons D electrons

23 105 Which element naturally occurs as a diatomic molecule? A K B C C Zn D H 106 A neutral atom of aluminum-27 contains A 14 protons and 13 neutrons B 13 electrons, 13 protons, and 14 neutrons C 13 protons and 27 electrons D 13 electrons, 14 protons, and 13 neutrons 107 What is the main similarity among elements in group 2? A Chemical properties B Atomic radius C Boiling point D Mass number 108 Which represents an atom of calcium? A 1 B 4 C 3 D How many valence electrons does a neutral atom of silicon have? A 6 B 3 C 4 D 5

24 110 The net charge on an aluminum ion is +3 because there are A 13 protons and 10 electrons in the atom B 10 neutrons and 13 electrons in the atom C 10 protons and 13 electrons in the atom D 13 protons and 10 neutrons in the nucleus 111 One indicator that electrons in atoms are limited to specific energy levels is that A atoms move faster when heated B the light given off by atoms is all at the same wavelength C light emitted from excited atoms occurs only at specific wavelengths D the Doppler effect shows a shift in wavelength for H-atom light 112 A scientist has found the following isotope of oxygen: How many neutrons are present in this isotope? A 19 B 11 C 27 D Which of the following is a mixture? A Glucose B Carbon C Distilled water D Air 114 Bonding between two elements of equal electronegativity would be A metallic in character B 100% covalent C 50% ionic D primarily ionic

25 115 At room temperature, chlorine exists as a gas, bromine exists as a liquid, and iodine exists as a solid. The physical states of these elements indicate that melting point A is constant within group 17 elements B increases from top to bottom within group 17 elements C is independent of periodic position D decreases from top to bottom with group 17 elements 116 The elements that are characterized by the presence of an incomplete d sublevel are called A halogens B transition elements C lanthanoids D alkali earth metals 117 Which of these best describes the difference between the formulas for nitrogen monoxide and nitrogen dioxide? A Nitrogen dioxide has one fewer atom of oxygen. B Nitrogen dioxide has one more atom of nitrogen. C Nitrogen monoxide has one fewer atom of oxygen. D Nitrogen monoxide has one more atom of nitrogen. 118 A chloride ion (Cl - ) has the same number of electrons as a neutral atom of A sulfur B fluorine C argon D bromine

26 119 Which of the following is most likely the electronegativity value for chlorine? A 2.3 B 4.2 C 3.0 D Atoms of the noble gases are generally inert because A they are too large to react B they are not charged C their outer electron levels are filled D they are neutral atoms 121 A 220 B 308 C 132 D When compared to sulfur-32, sulfur-34 has more A neutrons B protons C bonding configurations D energy levels 123 What are the numbers of protons, neutrons, and electrons in an isotope of titanium with a mass number of 50? A 50 p, 22 n, 50 e B 22 p, 28 n, 22 e C 22 p, 22 n, 28 e D 28 p, 22 n, 22 e

27 124 Place the following models about the structure of the atom in the order that they were developed: 1. Planetary model 2. Quantum mechanical model 3. Solid sphere model A 2, 3, 1 B 1, 2, 3 C 3, 1, 2 D 1, 3, In HNO3, the oxidation state of hydrogen is +1 and the oxidation state of oxygen is -2. Therefore, the oxidation state of nitrogen is A +3 B +4 C -1 D A sodium atom has an electron configuration of 1s 2 2s 2 2p 6 3s 1. If the sodium atom becomes ionized, its new electron configuration will be the same as which element? A Lithium B Potassium C Neon D Magnesium 127 Which element is a noble gas? A Nitrogen (N) B Xenon (Xe) C Fluorine (F) D Hydrogen (H) 128 Which set of coefficients will balance this equation? A 2, 6, 2 B 3, 1, 1 C 3, 2, 3 D 2, 3, 2

28 129 According to the periodic table, Mg will most likely react with elements in which of these groups? A 17 B 18 C 3 D Which of the following particles has a positive one (+1) charge? A Proton B Alpha C Neutron D Electron 131 After 1911, most scientists accepted the theory that the nucleus of an atom was very dense and very small and had a positive charge. What led scientists to accept this theory? A Scientists before 1911 used the scientific method of inquiry improperly. B Dalton s theory of the atom was over 100 years old. C A new model proved that the quantum theory of the atom was inaccurate. D Rutherford did an experiment firing alpha particles at a thin piece of gold foil. 132 In order to determine the identity of a substance, a student listed the following properties. Which of the following is a chemical property? A Oxidizes in air B Dissolves in water C Conducts an electric current D Attraction to a magnet 133 Iodine-131 is a radioactive isotope with a half-life of 8 days. How many grams of a 64 g sample of iodine-131 will remain at the end of 24 days? A 48 g B 8 g C 32 g D 56 g

29 134 An atom contains 70 protons, 70 electrons, and 99 neutrons. What is the mass number? A 140 B 70 C 239 D Which of these elements has the smallest atomic radius? A Sulfur (S) B Sodium (Na) C Oxygen (O) D Beryllium (Be) 136 What is the mass of one mole of CO2? A 44 g B 24 g C 56 g D 28 g 137 An example of a chemical property is A mass of a substance per unit volume B point where solid becomes liquid C tendency to undergo oxidation D ability to dissolve in solution 138 Which of the following is a chemical change? A Copper metal is stretched into a long wire. B Salt is dissolved in water. C Gasoline combusts in an engine. D Water is boiled on a stove. 139 Based on its position in the periodic table, the element sulfur would be expected to have how many valence electrons? A 4 B 16 C 8 D 6

30 140 Potassium (K) has a smaller atomic mass than argon (Ar) even though the atomic number of potassium is larger than the atomic number of argon. Which of the following best accounts for this observation? A It is easier for a potassium atom to lose an electron than it is for an argon atom. B At STP, potassium is in the solid phase, but argon is a gas. C The most common isotopes of argon have more protons than the most common isotopes of potassium. D The most common isotopes of potassium have fewer neutrons than the most common isotopes of argon. 141 A student hypothesizes that bromine (Br) has different chemical properties from krypton (Kr). The periodic table supports this hypothesis by indicating that A one mole of bromine is heavier than one mole of krypton B bromine and krypton have different numbers of valence electrons C bromine is a metal while krypton is a nonmetal D bromine and krypton are members of the same family 142 A chemist is examining an unidentified element sample with oxidation states of +2, +3, and +6. The element has a shielding effect similar to that of potassium (K). Which statement about the unidentified element is most likely true? A It is a transition metal from the same period as potassium. B It is a mix of three unstable isotopes of potassium. C It is one of the heaviest elements in potassium s group. D It has the same number of neutrons as potassium. 143 The picture shows a small section of elements from the periodic table. Which element has one more proton than element X? A 3 B 1 C 4 D 2

31 144 If a sample has a mass of g and a volume of 51 ml, what is its density? A 250 g/ml B 2.5 g/ml C g/ml D g/ml 145 Arrow number 1 should be labeled A Increases B Remains Constant C Fluctuates D Decreases 146 What subatomic particles are located in the orbital of an atom? A Protons and Electrons B Neutrons C Protons and Neutrons D Electrons 147 What is the electron configuration for helium? A 1s 1 B 1s 1 2s 2 C 1s 2 D 1s 1 2s 1

32 148 What is the electron configuration of Cl -? A 1s 2 2s 2 2p 6 3s 2 B 1s 2 2s 2 2p 6 3s 2 5p 3 C 1s 2 2s 2 2p 6 3s 2 3p 6 D 1s 2 2s 2 2p 6 3s 2 3p Which scientist created a model that took the place of Bohr's model of the atom? A Werner Heisenberg B Louis de Broglie C Max Planck D Henry Moseley 150 Which of the following elements is classified as a metal? A Element 3 has a higher electronegativity and has 7 electrons in the outer shell. B Element 1 loses valence electrons easily and is very ductile. C Element 4 is in the form of a liquid at room temperature and is transparent. D Element 2 is brittle and forms oxides that are acidic. 151 The electron configuration for magnesium is A 1s 2 2s 2 2p 6 3s 2 3p 2 B 1s 2 2s 2 2p 6 3s 1 C 1s 2 2s 2 2p 6 3s 1 D 1s 2 2s 2 2p 6 3s What function does an electron play in a chemical reaction? A Identity B Negative charge C Bonding D Nuclear stability

33 153 Which two elements have the same number of electron shells? A Lithium and argon B Helium and neon C Magnesium and sulfur D Potassium and sodium 154 Proton is to positive as electron is to A orbital B neutral C positive D negative 155 Of the following elements found in the halogen family, which one is the heaviest? A Iodine B Fluorine C Bromine D Polonium 156 All of the following elements are alkali metals EXCEPT A Helium B Hydrogen C Beryllium D Boron 157 The electron configuration for hydrogen is A 1s 2 2s 1 B 1s 2 2s 2 C 1s 2 D 1s 1

34 158 Which elements would always be classified as metals? A Elements W and Y B Elements V, W, and Y C Elements Z and X D Elements V, X, and Z 159 Which element would have the general electron configuration of ns 2 np 5, where "n" stands for the principle energy level? A Be B Cl C Sr D Cd 160 If you add an electron to an element in the halogen family, then the element will have the same number of electrons as a A alkaline earth metal B transition metal C alkali metal D noble gas 161 Arrow number 2 should be labeled A Decreases B Fluctuates C Remains Constant D Increases

35 162 1s 2 2s 2 2p 6 3s 2 3p 6... Complete the above electron configuration for calcium. A 3d 1 4s 1 B 4s 2 4p 1 C 3d 1 D 4s Which model is missing from the Quantum Models diagram? A Nature of Energy B Establishment of Matter C Energy Levels D Nuclear Structure 164 Using the chart, which element is represented by number 1? A Neon B Sodium C Silicon D Magnesium

36 165 Which historical model does number 3 represent on the timeline? A Initial idea of atom is established B Energy levels established in planetary model C Plum pudding model due to discovery of the electron D Periodic table is arranged by atomic number 166 On the periodic table, as you move from right to left, arrow 2, the ionization energy A increasing B fluctuating C remains constant D decreasing

37 167 1s 2 2s 2 2p? What number should replace the question mark in the electron configuration for nitrogen? A 2 B 4 C 1 D After seconds, 3.75 grams of an original 30 gram sample of Fermium-253 remains. What is the half-life of the sample? A seconds B seconds C seconds D seconds 169 A student observes a metalloid element with 5 electrons. What is the electron configuration of the element? A 1s 2 2s 2 B 1s 2 2s 2 2p 3 C 1s 2 2s 2 2p 1 D 1s 2 2s 2 2p 2

38 170 What historical model should be placed on the timeline at number 1? A Plum pudding model due to discovery of the electron B Periodic table is arranged by atomic number C Initial idea of atom is established D Energy levels established in planetary model 171 What subatomic particles are located in the nucleus of an atom? A Electrons and neutrons B Protons and neutrons C Electrons and quarks D Neutrons and photons

39 172 Number 2 should be replaced with the which historical model? A Plum pudding model due to discovery of the electron B Energy levels established in planetary model C Periodic table is arranged by atomic number D Initial idea of atom is established 173 Which student completed the electron configuration for a neutral element of argon correctly? A Student 4 B Student 3 C Student 5 D Student 1

40 174 Student 4 wrote the electron configuration for which neutral element? A Aluminum B Silicon C Sulfur D Potassium 175 What type of ionizing radiation can penetrate through paper, skin, and wood? A Alpha particles B Beta particles C Microwaves D Gamma rays 176 What type of charge will a halogen most likely have? A 1+ B 0 C 2+ D Which element has the electron configuration of 1s 2 2s 1 A Carbon B Lithium C Beryllium D Boron 178 What is a chemical property of a metal? A Good oxidizing agent B Forms oxides that are basic C Shares valence electrons easily D Possesses metallic luster

41 179 The information in the figure supports which theory? A Planetary Model B Atomic theory of matter C Quantum mechanical model D Nuclear Model 180 Which statement about the shielding effect in elements is correct? A Lithium has more of a shielding effect than beryllium. B Helium has more of a shielding effect than neon. C Boron and aluminum have the same shielding effect. D Copper and titanium have the same shielding effect. 181 The information in the figure was established by which scientist? A Ernest Rutherford B Democritus C J. J. Thomson D John Dalton 182 1s 2 2s 2 2p? What number should replace the question mark in the electron configuration for boron? A 3 B 2 C 4 D 1

42 183 If an atom has a size of 10-10, then the size of the protons in the atom must be A smaller than the atom but larger than the neutrons B smaller than the electrons but larger than the neutrons C smaller than the neutrons but larger than the electrons D smaller than the atom but larger than the electrons 184 The element represented by number 2 is A sulfur B sodium C silicon D magnesium 185 Neon is represented by element number A 5 B 3 C 2 D Which of the following elements has the highest ionization energy? A Argon B Phosphorus C Neon D Fluorine

43 187 How many valence electrons does boron contain? A 3 B 5 C 6 D Which atom or ion has the electron configuration of a noble gas? A K B Ca +2 C Mg +1 D Fe Completing the chart, what is the electron configuration for Cl? A 1s 2 2s 2 2p 6 3s 2 3p 5 B 1s 2 2s 2 2p 6 3s 2 3p 6 C 1s 2 2s 2 2p 6 3s 2 3p 4 D 1s 2 2s 2 2p 6 3s A student is observing an element that conducts electricity, is very reactive, makes a positive ion, and can make an alloy. What type of element is the student observing? A Valence B Metal C Inert gas D Halogen

44 191 Elements in Group 1 on the periodic table are most likely to react with elements in Group A 16 B 17 C 18 D Electrons are to bonding as neutrons are to A nuclear stability B atom identity C positive charge D orbital movement 193 1s 2 2s 2 2p 6 3s 2... Complete the above electron configuration for calcium. A 3p 6 4s 2 B 3p 6 4d 2 C 3p 6 3d 1 D 3p 6 3d 1 4s A 175 gram sample of Os-182 has a half-life of hours. After hours, how many grams of the sample remains? A g B g C g D g 195 A sample of element Z has 205 atoms with a mass of amu and 15 atoms with a mass of amu. What is the average atomic mass of element Z? A amu B amu C 0.95 amu D amu

45 196 Which element has the electron configuration of 1s 2 2s 2 A Beryllium B Boron C Lithium D Carbon 197 Which statement is correct? A Oxygen has less valence electrons than nitrogen. B Carbon and phosphorus have the same number of valence electrons. C Silicon has less valence electrons than sulfur. D Lithium has more valence electrons than neon. 198 What is the shown periodic table highlighting? A The periods of the periodic table B The identity of the periodic table C The teams of the periodic table D The groups of the periodic table

46 199 The trends seen in shielding on the periodic table indicates that arrow number one should be labeled A Decreases B Fluctuates C Increases D Remains Constant 200 What is the electron configuration of Si 4+? A 1s 2 2s 2 2p 6 3s 2 3p 2 B 1s 2 2s 2 2p 6 C 1s 2 2s 2 2p 6 3s 2 D 1s 2 2s 2 2p 6 3s Which statement about the trends in the atomic radius of elements is correct? A The radius of atoms decreases when moving from the top to the bottom of a group. B The radius of atoms increases when moving from the top to the bottom of a group. C The radius of atoms increases when moving from left to right on a certain period. D The radius of atoms decreases when moving from right to left on a certain period.

47 202 Student 1 wrote the electron configuration for which neutral element? A Argon B Magnesium C Aluminum D Silicon 203 The type of radiation observed in Type X is A Gamma B Beta C Microwave D Alpha 204 Which number represents an oxygen element? A Element 3 B Element 2 C Element 5 D Element 4

48 205 The atomic radius of aluminum is larger than A magnesium B indium C silicon D gallium 206 Beryllium has an electron configuration of 1s 2 2s 2. What is the electron configuration of Be 2+? A 1s 2 2s 4 B 1s 2 2s 1 C 1s 2 D 1s What is the nuclear charge of an atom with a mass number of 15 and an atomic number of 7? A +8 B +14 C +7 D Which statement is correct regarding the ionization of elements on the periodic table? A The element gold has a lower ionization energy level than the element platinum. B The element nitrogen has a higher ionization energy level than the element oxygen. C The element francium has electrons that can easily be removed from its atoms. D The element argon has electrons that can easily be removed from its atoms. 209 What is the electron configuration for neon? A 1s 2 2s 2 2p 6 3s 1 B 1s 2 2s 2 2p 6 3s 2 C 1s 2 2s 2 2p 5 D 1s 2 2s 2 2p 6

49 210 What type of radiation should replace the letter Y? A Beta B Microwave C Alpha D Gamma 211 What type of radiation is represented by W? A Gamma B Beta C Alpha D X-ray 212 Which of the following characteristics is a chemical property of nonmetals? A Outer shells contain 1-3 electrons B Forms oxides that are basic C Good oxidizing agents D Lower electronegativities

50 213 Arrow number 1 should be labeled A Remains Constant B Fluctuating C Increasing D Decreasing 214 Arrow number 2 should be labeled A Increases B Fluctuates C Decreases D Remains Constant 215 What is a physical property of a nonmetal element? A Opaque B Ductile C Brittle D Acidic oxide

51 216 Element number 2 is A Chlorine B Carbon C Calcium D Cobalt 217 What is element number 1? A Fluorine B Carbon C Iron D Chlorine 218 Nitrogen has how many valence electrons? A 6 B 4 C 3 D 5

52 219 The physical and chemical characteristics of four elements are being investigated. Which element is a nonmetal? A Element 1 is opaque, conducts heat, and is capable of forming an oxide that is basic. B Element 3 is a ductile element with 2 electrons in it's outer shell and is solid at room temperature. C Element 4 is an excellent reducing agent with a lower electronegativity and somewhat malleable. D Element 2 is a good oxidizing agent that is brittle and found in a gas state at room temperature. 220 Which of the following four elements are found in the same period? A Carbon, Nitrogen, Oxygen, and Sulfur B Lithium, Sodium, Potassium, and Rubidium C Boron, Silicon, Arsenic, and Tellurium D Calcium, Chromium, Iron, and Zinc 221 Which two elements have the same shielding effect? A Hydrogen and Lithium B Sodium and Sulfur C Aluminum and Arsenic D Beryllium and Chlorine 222 What is the average atomic mass of the three silicon isotopes rounded to four significant figures? A amu B amu C amu D amu

53 223 Which student found the correct electron configuration for a neutral element of calcium? A Student 1 B Student 2 C Student 3 D Student Which of the following elements has a principle quantum number of 5? A Iron B Potassium C Iodine D Boron

54 225 Which number represents the location of electrons in an atom? A 2 B 1 C 4 D The figure displays a section of a row from the periodic table. Which element has 18 neutrons if its mass number is 35? A Argon B Chlorine C Silicon D Sulfur

55 227 How many neutrons are found in an element of titanium? A 26 B 5 C 22 D Which of the following four elements are found in the same group? A Beryllium, Calcium, Strontium, and Barium B Potassium, Calcium, Scandium, and Titanium C Carbon, Phosphorus, Selenium, and Sulfur D Boron, Silicon, Germanium, and Antimony 229 Which chart correctly identifies the number of valence electrons for each element? A B C D

56 230 What subatomic particle is represented by Y? A Proton B Neutron C Quark D Electron 231 Element Y has 280 atoms with a mass of and 70 atoms with a mass of What is the average atomic mass (amu) of element Y? A amu B 9.60 amu C 2.80 amu D amu 232 Which family of elements do not like to bond with other elements because their electron shell is full? A Group 8A B Group 2A C Group 7A D Group 1A

57 233 How many protons are found in an element of Cesium? A 302 B 55 C 78 D A student has a g sample of Zn-71. The half life of the sample is 2.4 minutes. How much of Zn-71 remains after 14.4 minutes? A g B g C g D g 235 The scientist Ernest Rutherford found through experimentation that alpha particles were deflected when shot at a sheet of gold foil. Finding these three types of waves basically proved that A electrons move in a wave-like fashion B atoms can be neither created nor destroyed C atoms have a nucleus D electrons have a planetary-like orbit

58 236 The matter found represented by W is A an element B a heterogeneous mixture C a homogeneous mixture D a compound 237 Click on the element you would like to select. Be sure to select all correct elements. Which elements are classified as metals? Carbon Fluorine Potassium Beryllium Calcium Magnesium Chlorine 238 Which of the following elements has the highest level of electronegativity? A Fluorine E Sodium B Carbon F Beryllium C Phosphorous G Sulfur D Boron

59 239 What type of mixture is formed in the figure? A Homogeneous B Diatomic C Compound D Valence E Conglomerate F Heterogeneous 240 Student 5 wrote the electron configuration for which neutral element? A Argon B Chlorine C Potassium D Calcium