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162 Cards in this Set
- Front
- Back
Which of the following elements is in the same period as phosphorus? carbon, nitrogen, magnesium, oxygen
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Magnesium.
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Of the elements Pt, V, Li, and Kr, which is a nonmetal?
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Kr.
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The atomic number of an element is the total number of which particles in the nucleus?
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Protons.
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In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly? In, 49 p+ 49 e-. Cs, 55 p+ 132.9 e-. Zn, 30 p+ 60 e-. F, 19 p+ 19 e-.
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In, 49 p+ 49 e-.
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Which of the follwing is true about the electron configurations of the noble gasses? The highest s and p sublevels are completely filled. The highest occupied s and p sublevels are paritally filled. The electrons with the highest energy are in a d sublevel. The electrons with the highest energy are in an f sublevel.
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The highest occupied s and p sublevels are completely filled.
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The region of high probabilty of finding an electron.
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Atomic orbital.
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States the impossibility of knowing both velocity and position of a moving particle at the same time.
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Heisenberg uncertainty principle.
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The lowest energy level.
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Ground state.
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The tendency of electrons to enter orbitals of lowest energy first.
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Aufbau principle.
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The arrangement of electrons around atomic nucleus.
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Electron configuration.
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Each orbital has at most two electrons.
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Pauli exclusion principle.
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In the Bohr model of the atom, an electron in an orbit has a fixed _____.
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Energy.
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How does the energy of an electron change when the electron moves closer to the nucleus?
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It decreases.
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The principal quantum number indicates what property of an electron?
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Energy level.
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What is the shape of the 3p atomic orbital?
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Dumbbell.
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How many energy sublevels are in the second principal energy level?
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2.
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What is the maximum number of f orbitals in any single enrgy level in an atom?
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7.
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What is the maximum number of d orbitals in a principal energy level?
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5.
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What is the maximum number of orbitals in the p sublevel?
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3.
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What is the maximum number of electrons in the second principal energy level?
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8.
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When an electron moves from a lower to a higher energy level, the electron _____.
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Absorbs a quantum of energy.
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What types of atomic orbitals are in the third principal energy level?
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S, p, and d only.
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What is the next atomic orbital in the series 1s, 2s, 3s, 3p?
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4s.
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According to the aufbau principle, _____.
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Electrons enter orbitals of the lowest energy first.
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What is the number of electrons in the outermost energy level of an oxygen atom (valence electrons)?
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6.
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What is the elctron configuration of potassium?
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1s2 2s2 2p6 es2 4s1
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If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
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One electron in each orbital.
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Which color of visible light has the highest energy?
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Violet.
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How are the frequency and wavelength of light related?
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They are inversely proportional to each other.
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Emission of light from an atom occurs when an electron ____.
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Drops from a higher to a lower energy level.
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Give the electron configuration for calcium.
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1s2 2s2 2p6 3s2 3p6 4s2
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How many valence electrons does Bromine have?
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7.
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How many valence electrons does Platinum have?
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2.
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Why does the 4s get filled up before the 3d?
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There is an overlapping of energy levels, making the 4s actually closer to the nucleus.
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Give the electron configuration for Iron?
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1s2 2s2 2p6 3s2 3p6 4s2 3d6.
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Give the shorthand configuration for Iodine.
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(Kr) 5s2 4d10 5p5.
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What do the Lewis Dot Structures tell us about an atom?
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How many valence electrons there are.
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Give the quantum number set for the last electron in Arsenic.
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4 1 1 1/2.
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Give the electron configuration for Nitrogen.
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1s2 2s2 2p3.
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Give the shorthand configuration for Sodium.
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(Ne) 3s1.
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What do the horizontal rows on the Periodic Table tell us?
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Energy levels.
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What does the third number in the quantum number set tell us?
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Specific orbital.
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Give the quantum number for both of strontium's valence electrons.
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5 0 0 1/2 5 0 0 -1/2.
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give the shorthand configuration for Zirconium.
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(Kr) 5s2 4d2.
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How many third level electrons are in Phosphorus?
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5.
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How many dots would we place around Bromine in our Lewis Dot Structure?
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7.
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Draw the shorthand configuration for Argon.
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(Ne) 3s2 3p6.
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What would be the second quantum number in the set for a 4p electron?
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1.
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How many dots would be placed around Uranium in the Lewis Dot Structure?
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2.
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How many maximum electrons can fit in the f section?
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14.
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The atomic number of an element is the toal number of which particles in the nucleus?
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Protons.
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How does atomic radius change from top to bottom in a group in the periodic table?
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It tends to increase.
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How does atomic radius change from left to right across a period in the periodic table?
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It tends to decrease.
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What element in the second period has the largest atomic radius?
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Lithium.
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Which of the following elements has the smallest atomic radius?
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Chlorine.
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What is the charge of a cation?
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A positive charge.
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Which of the following statements is true about ions?
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Anions form when an atom loses protons.
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The metals in Groups 1A, 2A, and 3A ____.
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Lose electrons when they form ions.
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Which of the following statements is NOT true about ions?
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When a cation forms, more electrons are transfered to it.
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In which of the following sets are the charges given correctly for all the ions? Na+, Mg+, Al+. K+, Sr2+, O-2
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K+, Sr2+, O-2.
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What is the element with the highest electronegativity value? cesium, helium, calcium, fluorine.
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Fluorine.
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Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
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Increase in atomic size.
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Which of the following elements has the smallest ionization energy?
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Potassium.
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Electronegativity generally increases from ____ to ____ across a period.
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Left to right.
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As you move from left to right across the second period of the periodic table ____.
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Ionization energy increases.
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The atomic number of an element is the toal number of which particles in the nucleus?
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Protons.
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How does atomic radius change from top to bottom in a group in the periodic table?
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It tends to increase.
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How does atomic radius change from left to right across a period in the periodic table?
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It tends to decrease.
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What element in the second period has the largest atomic radius?
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Lithium.
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Which of the following elements has the smallest atomic radius?
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Chlorine.
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What is the charge of a cation?
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A positive charge.
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Which of the following statements is true about ions?
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Anions form when an atom loses protons.
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The metals in Groups 1A, 2A, and 3A ____.
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Lose electrons when they form ions.
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Which of the following statements is NOT true about ions?
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When a cation forms, more electrons are transfered to it.
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In which of the following sets are the charges given correctly for all the ions? Na+, Mg+, Al+. K+, Sr2+, O-2
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K+, Sr2+, O-2.
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What is the element with the highest electronegativity value? cesium, helium, calcium, fluorine.
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Fluorine.
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Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
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Increase in atomic size.
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Which of the following elements has the smallest ionization energy?
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Potassium.
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Electronegativity generally increases from ____ to ____ across a period.
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Left to right.
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As you move from left to right across the second period of the periodic table ____.
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Ionization energy increases.
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Of the following elements, which one has the smallest ionization energy?
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Aluminum.
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How many valence electrons are in an atom of phosphorus?
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5.
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How many valence electrons are in an atom of magnesium?
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2.
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How many valence electrons does a helium atom have?
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2.
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How many valence electrons are in a silicon atom?
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4.
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What is the name given to the electrons in the highest occupied energy level of an atom?
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Valence electrons.
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What is the charge on the strontium ion?
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2+.
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How many electrons does barium have to give up to achieve a noble-gas electron configuration?
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2.
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Which of the following elements does not form an ion with a charge of 1+?
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Fluorine.
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How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
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3.
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Which of the following occurs in an ionic bond?
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Oppostiely charged ions attract.
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What is the net charge of the ionic compound calcium fluoride?
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0.
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Which of the following particles are free to drift in metals?
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Electrons.
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What is the basis of a metallic bond?
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The attraction of metal ions to mobile electrons.
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How do atoms achieve noble-gas electron configuration in single covalent bonds?
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Two atoms share one electron each.
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why do atoms share electrons in covalent bonds?
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To attain a noble-gas electron configuration.
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Which of the following elements, when bonded to itself, are held together by triple covalent bonds/
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Nitrogen.
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Valence electrons that do not participate in bonding in diatomic oxygen molecules?
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Unshared pair.
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Which of the following diatomic molecules is joined by a double covalent bond?
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O2.
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A molecule with a single covalent bond is _____.
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Cl2.
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How many electrons can occupy a single molecular orbital?
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2.
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According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
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Pairs of valence electrons.
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Experimental evidence suggests that the H-C-H bond angles in ethene, C2 H4 are
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120 degrees.
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What type of hybrid orbital exists in the methane (CH4) molecule?
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sp3.
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What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom (ex. C2Cl2)?
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sp.
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If two identical carbon atoms bond together, they form what type of bond?
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Nonpolar covalent.
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The B-F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is
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Ionic.
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In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
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8 electrons.
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Compared with nonmetals, the number of valence electrons in metals is generally.
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Smaller.
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What is the hybridization of the central atom in PF3?
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sp3.
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What is the molecular geometry of water?
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Bent.
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What is the domain geometry of C02?
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Linear.
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What is the hybridization of the each carbon in C2H4?
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sp2
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What sublevels are involved in valence electrons?
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s and p.
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A physical blend of two or more components.
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Mixture.
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Part of a sample having unifrom compostition and properties.
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Phase.
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Not uniform in composition.
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Heterogeneous mixture.
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A substance formed in a chemical raction.
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Product.
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Starting substance in a chemical reaction.
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Reactant.
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An example of an extensive property of matter.
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Mass.
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Evaporation is a ____ change.
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Physical.
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Air cannot be classified as a ____.
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Substance.
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Soil is a ____ mixture.
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Heterogeneous.
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A ____ mixture cannot be considered a single phase.
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Heterogeneous.
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____ mixtures are known as solutions.
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Heterogeneous.
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Air is a ____ misture.
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Heterogeneous.
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Salt Water is a ____ mixture.
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Homogeneous.
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____ are substances.
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Compounds.
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Silver is a ____.
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Substance.
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What is one difference between a mixture and a compound?
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A compound can only be seperated into its components by chemical means.
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In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the ____ is a reactant.
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Sucrose.
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Fermenting of cheese is not a ____ change.
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Physical.
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Decomposing _____ involve a physical change.
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Doesn't.
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When paper turns yellow-brown upon exposure to sunlight, what type of chnage is likely taking place?
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A chemical change.
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A fracture formation ____ indicate that a chemical change may have taken place.
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Doesn't.
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What happens to matter during a chemical reaction?
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Matter is neither destroyed or created.
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The total mass of the reactants ____ the total mass of the products.
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Equals.
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Who was the man who lived from 460BC-370BC and was among the first to suggest the idea of atoms?
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Democritus.
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Which theory included that atoms of the same element are always identical?
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Dalton's Atomic Theory.
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In ____ particles, the mass of a neutron nearly equals the mass of a proton.
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Subatomic.
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Who conducted experiments to determine the quntity of charge carried by an electron?
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Millikan.
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All atoms are ____.
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Neutral, with the number of protons equaling the number of electrons.
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As a consequence of the discover of the nucleus by ____, Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
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Rutherford.
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The atomic number of an element is the total number of ____ particles in the nucleus.
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Protons.
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What does the number 84 in the name krypton-84 represent?
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The mass number.
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Isotopes of the same element have different ____.
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Numbers of neutrons.
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Determine the number of neutrons in 16 O.
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8.
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How many protons, electrons, and neutrons does an atom with the atomic number 50 and mass number 125 contain?
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50 protons, 50 electrons, 75 neutrons.
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True or false: Atoms are mostly empty space.
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False.
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How is the number of neutrons in the nucleus of an atom calculated?
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Subtract the number of protons from the mass number.
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How many neutrons does 238/92 U have?
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146.
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What unit is used to measure weighted average atomic mass?
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Amu.
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True or false: Neutrons are located in the nucleus of an atom.
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False.
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The average atomic mass of an element depends upon the ____.
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Mass and relative abundance of each isotope of that element.
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What particle is emitted in alpha radiation?
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Helium nucleus.
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What is the change in the atomic number when an atom emits an alpha particle?
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Increases by 2.
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What is the change in atomic number caused by the emission of gamma radiation?
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Remains the same.
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What symbol is used for beta radiation?
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0/-1 e
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What is the change in atomic mass number when an atom emits an alpha particle?
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Decreases by 4.
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If an isotope decays by the process of beta emission, ____.
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The atomic number changes.
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Nuclear fusion ____.
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Takes place in the sun.
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What device was created by JJ Thomson in his discovery of the electron?
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Cathode ray tube.
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