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Nylffn1997

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this is an exam with 60  questions i am completing half of them mylself it is a timed test 

34 chemistry multiple choice.docx 

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QUESTION 1 1. Who is considered the 'father' of modern chemistry? Ernest Rutherford Erwin Schrödinger Antoine Lavoisier John Dalton 3 points QUESTION 2 1. Who discovered that a dense positively charged atomic nucleus is at the core of every atom? Ernest Rutherford Erwin Schrödinger Antoine Lavoisier John Dalton 3 points QUESTION 3 1. In which time period did Ancient Greek philosophers propose that all matter was composed of four fundamental substances: earth, air, water, and wind? 8000 BC – 1000 BC 1000 BC – 450 BC 300 BC – 1400 AD 1774 – 1794 AD Time period 1 Time period 2 Time period 3 Time period 4 2. Time period 1 Time period 2 Time period 3 Time period 4 3 points QUESTION 4 1. Which model best represents JJ Thomson's model of the atom? Model 1 Model 2 Model 3 Model 4 3 points QUESTION 5 1. Which model best represents Rutherford's model of the atom? Model 1 Model 2 Model 3 Model 4 3 points QUESTION 6 1. Which of the following statements is correct? All atoms are electrically neutral. All atoms are negatively charged. All isotopes are positively charged. All elements have an electrical charge. 3 points QUESTION 7 1. Which of the following statements correctly describes the relative charge of the subatomic particles? protons have the same charge as neutrons protons and electrons have equal but opposite charges protons and neutrons have equal but opposite charges electrons and neutrons have equal but opposite charges 3 points QUESTION 8 1. Which factor contributes most to the size of an atom? the atom's number of protons the atom's number of neutrons the atom's number and arrangement of electrons the atom's number of protons, neutrons and electrons all contribute equally to the atomic size 3 points QUESTION 9 1. Which of the following is the most accurate definition of an element? a pure substance that cannot be separated into simpler substances by physical or chemical means the most basic building block of matter the particles that make up atoms a combination of two or more atoms that are chemically combined 3 points QUESTION 10 1. Atoms of the same element are alike because they must have the same number of: electrons protons neutrons both protons and electrons 3 points QUESTION 11 1. Compare an electrically neutral atom of oxygen and an isotope of oxygen. QUESTION 12 1. Compare the two atoms: 188 "X" and 178 "Y". How are these atoms related? They are atoms of different elements They have the same number of neutrons They have different numbers of protons They are isotopes of the same element 3 points QUESTION 13 1. If two atoms have the same atomic numbers but different mass numbers, then they can be considered atoms of the same element. True False 2 points QUESTION 14 1. Electromagnetic forces are the predominant force in holding protons and neutrons together in the nucleus of an atom. True False 2 points QUESTION 15 1. The nucleus of the atom is held together by the mutual attraction of the positively charged protons and the negatively charged neutrons. True False 2 points QUESTION 16 1. Rutherford's model and Bohr's model are alike in that they both: reasoned that the nucleus was dense and positive and the electrons were negative and orbited the nucleus reasoned that the nucleus was negatively charged and the electrons were positively charged shared the idea of exact electron locations within the atom agreed that the "plum pudding" model of the atom was the only explanation that supported the available data 3 points QUESTION 17 1. The "fatal flaw" in Rutherford's model of the atom, which was corrected by Bohr's model, was the idea that, if the electrons were: orbiting the nucleus, changing direction and thus giving off energy, the electrons would lose all energy and collapse into the nucleus moving so rapidly, they would spiral away from the nucleus and be lost not moving they could not maintain their distance from the nucleus located too far from the nucleus they would not be attracted 3 points QUESTION 18 1. Match the scientist to his contribution to quantum theory: theorized that light energy can either be released or absorbed in discrete packets known as "quanta" Read Answer Items for Question 18 described all radiant energy as behaving like a stream of particles Read Answer Items for Question 18 Answer A. Albert Einstein Heisenberg C. Max Planck D. Louis deBroglie E. Niels Bohr B. Werner proposed the Uncertainty Principle Read Answer Items for Question 18 suggested that electrons could move as particles and as waves Read Answer Items for Question 18 theorized that electrons moved about the nucleus in fixed orbits; Known as the "Planetary Model" Read Answer Items for Question 18 5 points QUESTION 19 1. Max Planck contributed to the development of quantum theory with his theory of "quanta." Which of the following indicates how Planck arrived at his theory of "quanta"? Atoms of neon gas and sodium vapor are excited electronically, subsequently emitting different colors; red-orange and yellow, respectively. A solid black object is heated on a stove burner. Depending on the length of time exposed to the heat of the burner, the black object will appear red when containing less heat energy and appear white when containing more heat energy. The surface of a clean piece of metal is exposed to a light source. During exposure, the surface of the metal emits electrons. Electrons are passed through a crystal and are diffracted. 3 points QUESTION 20 1. The quantum numbers n, , ml, and ms give the exact location of an electron thus disproving Schrödinger's theory that it is only possible to discuss the location of an electron in terms of probability and electron density. True False 2 points QUESTION 21 1. The wave mechanical model of electron behavior helped to explain: that an electron can be defined by its energy, frequency or wavelength that electrons always acted as particles and never like waves why Rutherford's model was superior to Bohr's in explaining electron behavior why electrons can never be moved from their original orbits 3 points QUESTION 22 1. How many more atomic orbitals does a "d" sublevel hold than a "p" sublevel? 2 4 6 8 3 points QUESTION 23 1. The sublevel that has the largest number of differently shaped orbitals is the f sublevel. True False 2 points QUESTION 24 1. The "s" atomic orbital has only one possible value for the m quantum number True False 2 points QUESTION 25 1. Which of the following electron "address" locations represents an electron with the highest energy? 6s2 4d7 4f1 5p6 3 points QUESTION 26 1. The fact that the 2s orbital would fill with electrons before the 2p orbital would accept electrons is an application of: the Aufbau principle Hund's rule the Pauli exclusion principle Schrödinger's equation 3 points QUESTION 27 Describe the orbital notation and electron configuration notation to describe the placement of all of the electrons in an atom of Nitrogen. QUESTION 28 1. What is the energy of a single photon of blue light with a wavelength of 488 nm? 3.24 x 10-31 J 3.24 x 10-40 J 4.08 x 10-28 J 4.08 x 10-19 J 3 points QUESTION 29 1. Different elements emit different emission spectra when they are excited because each type of element has a unique energy level systems. Each element has a different set of emission colors because they have: different nuclear masses different energy level spacing different atomic masses static energy levels that trap and keep electrons at ground level 3 points QUESTION 30 1. What is the location of the last electron of the sodium atom? 3s0 3s2 2p6 3s1 3 points QUESTION 31 1. Match the following energy levels with the proper description. 4d Read Answer Items for Question 31 5f Read Answer Items for Question 31 7s Read Answer Items for Question 31 Answer A. Contains the sublevel with the least number of atomic orbitals B. Contains the sublevel that may hold up to 6 electrons when it is full C. Contains the highest sublevel D. Contains the lowest main energy level 5:00 PM Read Answer Items for Question 31 4 points QUESTION 32 1. Areas in which discrepancies were observed between classical mechanics and quantum mechanics are: blackbody radiation and the photoelectric effect. True False 2 points QUESTION 33 1. A single particle's motion can be analyzed by quantum mechanics, but quantum mechanics cannot describe multi-particle systems analytically, as there are too many variables involved in the calculations. True False 2 points QUESTION 34 1. Quantum mechanics is more effective at explaining phenomena that are of "normal" size (larger than a molecule and smaller than a planet), at a "normal" temperature (anywhere close to room temperature), and going a normal speed (from 0 m/s- to anything significantly less than the speed of light). True False 2 points
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