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PRACTICE - TEST on Atomic Structure Name: ______________________ 1) Complete the table below – Note that the particles are not is the same order: 3 points Charge Location AMU Neutron Electron Proton 2) Complete the table below -- 5 points Isotope Symbol Element Name 15 N Atomic Number Number of Protons Number of Neutrons Mass Number Nitrogen Number of Electrons 15 28 Al Calcium 21 39 74 3) Complete the table below -- 5 points Atomic # F P Mg P+ e- E1 E2 E3 E4 Ve- Group N-m 4) Draw the Lewis Structures for the following neutral atoms. 6 points C F Si He Ga Ba 5) Complete the boxes below. Be sure to include the electron configuration on the correct energy levels. Draw the Lewis Structure of each resulting atom. 8 points Oxygen - 16 Argon - 40 - e = ___ P+ = _____ N0 = _____ e- =____ Lewis Structure P+ = _____ N0 = _____ 1 2 1 3 Atomic # ____ Mass # ____ 2 3 Atomic # ____ Mass # ____ Lewis Structure 6) What is the electron configuration of the following elements? (USE 1s2, 2s2…. Configuration) 3 points MgBrAg- 7) Fill in the blanks using one of the following elements. Please note that each element may be used once, more than once, or not at all. 16 points K, Ca, Ga, C, As, O, Cl, Kr ________ is an example of metal ________ is an example of a nonmetal ________ is an example of a metalloid ________ has an atomic number of 8 ________ has 6 total electrons ________ has 6 valence electrons ________ has 1 valence electrons ________ has 19 protons ________ is in period 4 ________ is in period 2 ________ is in group 5A ________ is in group 4A ________ is an Alkaline Earth Metal ________ is a Nobel Gas. ________ is a Halogen ________ is an Alkali Metal 8) Look at each pair of elements below, select (circle) which element has the larger atomic radii: Be or Ca Na or P N or B 3 points 9) Look at each pair of elements below, select (circle) which element has the higher ionization energy: C or Si F or Br N or Li 3 points 10) Look at each pair of elements below, select (circle) which element has the higher electronegativity: O or Se P or Mg N or F 3 points 11) TRUE or FALSE - there is no such thing as a 2p orbital. 12) TRUE or FALSE - the 3d orbital can hold a maximum of 6 electrons 13) TRUE or FALSE - electrons can be found between the energy levels (between E2 & E3 = E 2.5) Moving from left-to-right across a period (row) of the periodic table, (40-45 14) 15) 16) 17) 18) 19) TRUE or FALSE - the atomic mass increases by ONE from element to element TRUE or FALSE - the elements become more non-metallic TRUE or FALSE - the ionization energy of the elements generally decreases TRUE or FALSE - the elements are arranged according to increasing atomic number TRUE or FALSE - each element has a unique number of neutrons TRUE or FALSE - the atomic radius of the elements generally decreases Directions: Match each item (a-p) with the correct statement below (16-31). NOTE: Each item may be used once, more than once, or not at all. a b. c. d. e. atom proton neutron electron nucleus f. g. h. i. j. atomic number average atomic mass mass number isotope atomic mass unit k. m. n. o. p. group period electronegativity ionization energy atomic radius 20. ____ the smallest particle of an element that retains the properties of that element 21. ____ vertical column in the periodic table 22. ____ the total number of protons and neutrons in the nucleus of an atom 23. ____ the identity of an element is determined by the number of ___________ in the nucleus 24. ____ one-half the distance between the nuclei of two atoms when the atoms are joined 25. ____ a negatively charged subatomic particle 26. ____ a positively charged subatomic particle 27. ____ the weighted average of the masses of the isotopes of an element 28. ____ the central part of an atom, containing protons and neutrons 29. ____ the number of protons in the nucleus of an element 30. ____ atoms with the same number of protons, but different numbers of neutrons in the nucleus 31. ____ energy required to remove an electron from an atom 32. ____ horizontal row in the periodic table 33. ____ ability of an atom to attract electrons when the atom is in a compound 34. ____ a subatomic particle with no charge 35. ____ almost all of the mass of the atom is contained in the __________ 36) Neon is in period _____, group ______, has _____ protons, and is considered a __________________ For the following questions, put your answer in the box ___ at the beginning of the question. 37) ___ Use the periodic table to determine the number of electrons in a neutral atom of beryllium. 38) ___ Use the periodic table to determine the number of protons in an atom of bromine. 39) ___ What is the atomic number for an element with 35 neutrons and a mass number of 68? 40) ___ What is the mass number for a carbon atom that has 7 neutrons in its nucleus? 41) ___ How many neutrons are present in an atom of the isotope 42) ___ How many electrons are in the highest occupied energy level of a neutral neon atom? 43) ___ How many protons are present in an atom of Na-23? Sr ? _____ 44) Which of the following is true about subatomic particles? a. Electrons have no charge and have almost no mass. b. Protons are negatively charged and the lightest subatomic particle. c. Neutrons have a negative charge and are the lightest subatomic particle. d. Electrons have almost no mass compared to the protons _____45) All atoms are ____. a. neutral, with the number of protons equaling the number of electrons b. neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons c. positively charged, with the number of protons exceeding the number of electrons d. negatively charged, with the number of electrons exceeding the number of protons _____46) The nucleus of all atoms ____. a. always has the same number of neutrons and is considered neutral b. are positively charged because of the positive charge of the protons c. are negatively charged because of the negative charge of the neutrons d. are positively charged and it occupies the vast majority of the volume of the atom. _____47) The sum of the protons and electrons in an atom equals the ____. a. atomic number b. charge of the atom c. atomic mass d. mass number _____ 48) What does the number 11 in the name boron-11 represent? a. the atomic number c. the sum of the protons and electrons b. the mass number d. twice the number of protons _____ 49) Isotopes of the same element have different ____. a. numbers of neutrons b. numbers of protons c. numbers of electrons _____50) All atoms of the same element have the same ____. a. number of neutrons b. number of protons c. mass numbers d. atomic numbers d. mass _____ 51) What unit is used to measure weighted average atomic mass? a. photons b. picometers c. amu d. density _____ 52) Which of the following statements is NOT true? a. Atoms of the same element must always have the same mass b. Atoms of isotopes of an element have different numbers of neutrons. c. The nucleus of an atom has a positive charge. d. Atoms are mostly empty space. _____ 53) Which of the following would be an isotope of an element that had 17 protons, 18 neutrons and 17 electrons? a. 17 protons, 18 neutrons, 18 electrons c. 18 protons, 18 neutrons, and 17 electrons b. 17 protons, 18 neutrons, 16 electrons d. 17 protons, 17 neutrons, and 17 electrons _____ 54) How many protons, electrons, and neutrons does an atom with atomic number 75 and mass number 145 contain? a. 50 protons, 50 electrons, 75 neutrons c. 120 neutrons, 50 protons, 75 electrons b. 75 electrons, 50 protons, 50 neutrons d. 70 neutrons, 75 protons, 50 electron _____ 55) How do the isotopes Carbon-12 and Carbon-13 differ? a. Carbon-12 has one more electron than hydrogen-1. b. Carbon-12 has 12 neutrons; carbon-13 has 13 neutrons c. Carbon-13 has one more neutron than carbon-12 d. Carbon-13 has one more proton that carbon-12 _____ 56) The atomic mass of an element depends on the _______. a. Mass of each electron in that element b. Mass of each isotope of that element c. Relative abundance of protons in that element d. Mass and relative abundance of each isotope of that element _____ 57) In the Bohr model of the atom, an electron in an orbit has a fixed ____. a. position b. color c. energy d. size _____ 58) How does the energy of an electron change when the electron moves farther from the nucleus? a. It decreases. b. It increases c. It stays the same. d. It doubles. _____ 59) What is the maximum number of electrons in the first principal energy level (E1)? a. 2 b. 8 c. 18 d. 32 _____ 60) What is the number of electrons in the outermost energy level of an silicon atom? a. 2 b. 4 c. 6 d. 8 _____ 61) Emission of light from an atom occurs when an electron ____. a. becomes excited and jumps to a higher energy level c. is in its ground state b. relaxes and returns to its ground state d. is in its excited state _____ 62) Which of the following elements is in the same period as krypton? a. helium b. magnesium c. nitrogen d. bromine _____ 63) Electron configurations are arranged based upon_____? a. the lowest possible energy b. The number of protons in a neutral atom c. the highest possible energy d. The excitation and relaxation of the valence electrons _____ 64) Of the elements Fr, Sb, Al, and Rn, which is a metalloid? a. Fr b. Sb c. Al d. Rn _____ 65) Each period in the periodic table corresponds to ______. a. the number of valence electrons b. energy levels c. the mass d. protons and neutrons _____ 66) How does the atomic radius change from top to bottom in a group in the periodic table? a. it tends to decrease c. It first increases, then decreases b. it tends to increase d. It does not change, it will always be the same _____ 67) Which of the following increases with increasing atomic number in Group 2A? a. shielding effect b. ionic size c. ionization energy d. number of electrons _____ 68) Which of the following orbitals has the highest amount of energy? a. 3d b. 4p c. 4f d. 5s 69) Explain how you can use the periodic table of elements to determine the number of electrons in the outer most energy level. 2 points 70) Explain the process of electron excitation. 2 points 71) Which elements have similar properties to the element Chlorine (Cl)? 2 points 72) How do you know that these elements have similar properties to Chlorine? 2 points 73) Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope Z-19 with a mass number of 19.0 is 55.0% abundant; and the isotope Z-21 with a mass number of 21.0 is 45.0% abundant. Calculate the average ATOMIC MASS for element Z. 3 points