Please select a Team.

1. Please select a Team. • Females • Those that aren’t female

2. The order of elements in the modern periodic table is based on • the number of protons in the nucleus. • the electric charge of the nucleus. • the number of neutrons in the nucleus.

3. Atoms of elements that are in the same group are in the same • Horizontal row • Vertical column

4. Atoms of elements that are in the same group have the same number of • protons. • neutrons. • valence electrons. • protons and neutrons.

5. Which of the following elements is an noble gas? • A • B • C • D

6. Which of the following elements is an alkali metal? • A • B • C • D

7. Which of the following elements is an alkaline Earth metal? • A • B • C • D

8. Which of the following elements is an halogens? • A • B • C • D

9. Semiconductors are elements that • have large atomic masses but small atomic numbers. • do not form compounds. • can conduct heat and electricity under certain conditions. • are extremely hard.

10. Carbon and other nonmetals are found in which area of the periodic table? • on the left-most side • on the right side • in the middle column of the periodic table • in the bottom rows

11. Which is the p block? • A • B • C • D

12. Which is the s block? • A • B • C • D

13. Which is the f block? • A • B • C • D

14. Which is considered the d block? • A • B • C • D

15. Team Scores

16. In Mendeleev’s periodic table, elements in each column had similar • Physical properties. • Chemical properties. • Both of these • None of these

17. Magnesium (Mg #12) is located to the right of sodium (Na #11) because Mg has • fewer protons. • no neutrons. • no protons. • more protons.

18. As you move from left to right across the periodic table, elements • become less metallic. • have a lower atomic number. • have a lower atomic weight. • become more metallic.

19. Each column of the periodic table is • an element. • a group. • an isotope. • a period.

20. The periodic law states that elements that have similar properties appear • to the left of each other. • to the right of each other. • at every tenth element. • at regular intervals and then repeat.

21. What is the location of elements in the periodic table related to? • color • number of neutrons • atomic weight • electron configuration

22. Team Scores

23. Which of the following is not a type of orbital? • s • d • p • x

24. An electron jumps up or down to a new energy level when • the atom becomes charged. • the atom becomes unstable. • the electron’s location is pinpointed. • the atom gains or loses energy.

25. The number of energy levels filled in an atom is determined by • protons. • electrons. • neutrons.

26. Which of the following statements is not true? • An s orbital can hold two electrons. • Each of 5 dorbitals can hold up to two electrons. • Each of 7 forbitalscan hold up to three electrons. • Each of 3 porbitalscan hold two electrons.

27. Team Scores

28. An emission line spectrum is produced when an electron moves from one energy level • to a higher energy level. • to a lower energy level. • into the nucleus. • to another position in the same sublevel.

29. Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen • had no electrons. • did not release photons. • released photons of only certain energies. • could only exist in the ground state.

30. For an electron in an atom to change from the ground state to an excited state, • energy must be released. • energy must be absorbed. • radiation must be emitted. • the electron must make a transition from a higher to a lower energy level.

31. If electrons in an atom have the lowest possible energies, the atom is in the • ground state. • inert state. • excited state. • radiation-emitting state.

32. Which orbital is this? • s • p • d • f

33. Which orbital is this? • s • p • d • f

34. If each of these sub orbitals contains 2 electrons, what element is this? • B • N • F • Ne • Na

35. Team Scores

36. The electron in a hydrogen atom has its lowest total energy when the electron is in its • neutral state. • excited state. • ground state. • quantum state.

37. The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called • d orbitals. • p orbitals. • f orbitals. • s orbitals.

38. A spherical electron cloud surrounding an atomic nucleus would best represent • an s orbital. • a px orbital. • a combination of px and py orbitals. • a combination of an s and a px orbital.

39. The major difference between a 1s orbital and a 2s orbital is that • the 2s orbital can hold more than 2 electrons. • the 2s orbital has a slightly different shape. • the 2s orbital is at a higher energy level. • the 1s orbital can have only one electron.

40. The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are • s:2, p:4, d:6, and f:8. • s:1, p:3, d:5, and f:7. • s:2, p:6, d:10, and f:14. • s:1, p:2, d:3, and f:4.

41. Team Scores: 2 rounds left!!

42. The atomic sublevel with the next highest energy after 4p is • 4d. • 4f. • 5p. • 5s.

43. The atomic sublevel with the next highest energy after 3s is • 3d. • 2f. • 3p. • 4s.

44. In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons? • 3d1 4s2 • 4s3 • 3d3 • 4s2 4p1

45. Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau principle? • 1s 2s 2p 3s 4s 3p 3d 4p 5s • 1s 2s 2p 3s 3p 4s 3d 4p 5s • 1s 2s 2p 3s 3p 4s 4p 3d 4d • 1s 2s 2p 3s 3p 3d 4s 4p 5s

46. The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is • Mg (Z = 12). • C (Z = 6). • S (Z = 16). • Si (Z = 14).

47. The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is • 3. • 6. • 11. • 12.

48. Team Scores

49. Which of the following elements is an alkali metal? • Magnesium (# 12) • Fluorine (#9) • Titanium (#22) • Lithium (#3) • Neon (#10)

50. Which of the following elements is an alkaline-Earth metal? • Magnesium (# 12) • Fluorine (#9) • Titanium (#22) • Lithium (#3) • Neon (#10)