Reference no: EM13871893

1) Which of the statements about light is FALSE?
A) Light travels through space at a speed of 3.00 × 108 m/s.
B) Light travels much faster than sound.
C) A packet of light energy is called a photon.
D) A characteristic feature of light that determines its color is its wavelength.
E) All of the above statements are true.

2) The distance between adjacent wave crests is called:
A) wavelength.
B) frequency.
C) trough.
D) nu.
E) none of the above

3) The number of cycles of a wave that passes a stationary point in one second is called its:
A) wavelength.
B) frequency.
C) crest.
D) trough.
E) none of the above


4) Which among the following statements is TRUE?
A) The wavelength of light is inversely related to its energy.
B) As the energy increases, the frequency of radiation decreases.
C) As the wavelength increases, the frequency also increases.
D) Red light has a shorter wavelength than violet light.
E) none of the above

5) How are wavelength and frequency of light related?
A) Wavelength is one-half of the frequency.
B) Wavelength is double the frequency.
C) Wavelength increases as frequency increases.
D) Wavelength increases as the frequency decreases.
E) Wavelength is independent of frequency.

6) Which color of the visible spectrum has the shortest wavelength (400 nm)?
A) red
B) orange
C) green
D) violet
E) yellow


7) Which color of the visible spectrum has the longest wavelength (750 nm)?
A) red
B) orange
C) green
D) violet
E) yellow


8) Which color of the visible spectrum has photons with the most energy?
A) red
B) orange
C) green
D) violet
E) yellow

9) What is the correct order of the electromagnetic spectrum from shortest wavelength to longest?
A) Gamma Rays→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Radio Waves
B) Visible Light→Infrared Radiation→Microwaves→Radio Waves→Gamma Rays→X-rays→Ultraviolet Radiation
C) Radio Waves→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Gamma Rays
D) Gamma Rays→X-rays→Visible Light→Ultraviolet Radiation→Infrared Radiation→Microwaves→Radio Waves
E) Gamma Rays→X-rays→Infrared Radiation→Visible Light→Ultraviolet Radiation→Microwaves→Radio Waves

10) Which form of electromagnetic radiation has the shortest wavelength?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation


11) Which form of electromagnetic radiation has the longest wavelength?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation

12) Which form of electromagnetic radiation has the highest frequency?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation

13) Which form of electromagnetic radiation has the lowest frequency?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation

14) Which form of electromagnetic radiation has photons with the highest energy?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation

15) Which form of electromagnetic radiation has photons with the lowest energy?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation

16) What happens to an atom when it absorbs energy?
A) The atom stores the energy for later use.
B) The extra energy increases the speed of the electrons in their orbitals.
C) The atom re-emits the energy as heat.
D) The atom re-emits the energy as light.
E) none of the above


17) When sunlight is passed through a prism, what is observed?
A) continuous spectrum
B) nothing
C) bright spots and lines
D) white light
E) none of the above

18) When neon light is passed through a prism, what is observed?
A) continuous spectrum
B) nothing
C) bright spots or lines
D) white light
E) none of the above


19) Which statement below does NOT follow the Bohr Model?
A) When energy is absorbed by atoms, the electrons are promoted to higher-energy orbits.
B) When an atom emits light, electrons fall from a higher orbit into a lower orbit.
C) The energy emitted from a relaxing electron can have any wavelength.
D) Electrons exist in specific, quantized orbits.
E) none of the above

20) Which of the following statements about the quantum-mechanical model is FALSE?
A) Orbitals are a probability map of finding electrons.
B) Electrons do not behave as particles.
C) Orbitals are specific paths electrons follow.
D) Electron paths cannot be described exactly.
E) All of the above are correct statements.


21) The principal quantum number (n):
A) specifies the 3-D shape of the orbital.
B) specifies the subshell of the orbital.
C) specifies the maximum number of electrons.
D) specifies the principal shell of the orbital.
E) none of the above

22) The subshell letter:
A) specifies the 3-D shape of the orbital.
B) specifies the principal quantum number of the orbital.
C) specifies the maximum number of electrons.
D) specifies the principal shell of the orbital.
E) none of the above


23) How many subshells are there in the n = 4 principal shell?
A) 1
B) 2
C) 3
D) 4
E) not enough information

24) How many subshells are there in the n = 2 principal shell?
A) 1
B) 2
C) 3
D) 4
E) not enough information


25) The n = ________ principal shell is the lowest that may contain a d-subshell.
A) 1
B) 2
C) 3
D) 4
E) not enough information

26) Which subshell letter corresponds to a spherical orbital?
A) s
B) p
C) d
D) f
E) not enough information


27) Which subshell letter corresponds to a 4-leaf clover orbital pattern?
A) s
B) p
C) d
D) f
E) not enough information

28) Which statement is NOT true about "p" orbitals?
A) A subshell contains three "p" orbitals.
B) These orbitals are shaped like dumbbells.
C) A 3p orbital has a higher energy than a 2p orbital.
D) All three of these statements are true.
E) none of the above

29) The "d" subshell can hold a maximum of ________ electrons.
A) 2
B) 5
C) 6
D) 10
E) none of the above

30) How many electrons can exist in an orbital?
A) 1
B) 2
C) 3
D) 4
E) none of the above


31) The lowest energy orbital in the quantum-mechanical model is the:
A) zero orbital.
B) 1a orbital.
C) 1p orbital.
D) 1s orbital.
E) none of the above

32) "When filling orbitals of equal energy, electrons fill them singly first with parallel spins." This is known as:
A) Hund's rule.
B) Pauli exclusion principle.
C) Bohr's model.
D) Ground state.
E) none of the above

33) The subshell that has three orbitals and can hold up to six electrons is the:
A) s subshell
B) p subshell
C) d subshell
D) f subshell
E) none of the above

34) The subshell that has five orbitals and can hold up to ten electrons is the:
A) d subshell
B) f subshell
C) s subshell
D) p subshell
E) none of the above


35) Which orbital would the electron of a ground state hydrogen atom occupy?
A) 1s
B) 2p
C) 0s
D) 1p
E) none of the above

36) How many electrons are unpaired in the orbitals of carbon?
A) 12
B) 6
C) 4
D) 2
E) none of the above


37) How many electrons are unpaired in the orbitals of nitrogen?
A) 14
B) 5
C) 9
D) 3
E) none of the above

38) An accepted abbreviation format is to write an electron configuration that includes a noble gas symbol in brackets. If you were writing an electron configuration for a bromine atom, which elemental symbol would you place in the bracket?
A) He
B) Ne
C) Ar
D) Kr
E) Xe


39) Which element is represented by the electron configuration 1s22s22p2?
A) C
B) He
C) Be
D) O
E) none of the above

40) What is the electron configuration for Kr?
A) 1s22s22p63s23p43d104s24p6
B) 1s22s22p63s23p64s23d24p6
C) 1s22s22p63s23p64s23d104p6
D) 1s22s22p63s23p24s23d104p6
E) none of the above


41) What is the electron configuration for Ga?
A) 1s22s22p63s23p63d104s24p6
B) 1s22s22p63s23p64s23d104p1
C) 1s22s22p63s23p53d104s24p1
D) 1s22s22p63s23p64s24d104p1
E) none of the above

42) What is the electron configuration for P?
A) [Ar]3s23p64s23d104p3
B) [Ne]1s21p62s22p3
C) [Ne]3s23p3
D) [Ar]3s23p3
E) none of the above


43) Which one of the following is the correct orbital diagram for nitrogen?
A) ↑↓ ↓ ↓ ↑
B) ↓ ↑ ↑
C) ↑ ↑ ↑
D) ↑↓ ↑ ↑ ↑
E) none of the above

44) The element with a completely filled p-subshell is:
A) Na.
B) Al.
C) P.
D) Ar.
E) none of the above

45) What is the element in which at least one electron is in the d-orbital?
A) Ar
B) K
C) Ca
D) Sc
E) none of the above

46) How many core electrons are in a chlorine atom?
A) 1
B) 17
C) 10
D) 7
E) none of the above


47) How many valence electrons are in a chlorine atom?
A) 1
B) 17
C) 10
D) 7
E) none of the above

48) What do the alkali metals all have in common?
A) They all undergo similar reactions.
B) They all have similar physical properties.
C) They all form +1 ions.
D) They all have the same number of valence electrons.
E) all of the above


49) Which of the following elements has the electron configuration of 3s23p4 in its outermost shell?
A) Al
B) Si
C) S
D) Cl
E) none of the above

50) Chlorine and bromine have very similar chemical properties. This is best explained by the fact that both elements:
A) are gases.
B) are in period 3 of the Periodic Table.
C) have the same number of valence electrons.
D) have equal number of protons and electrons.
E) none of the above


51) Consider the electron configuration of the ion to determine which ion shown below has an incorrect ionic charge?
A) Al3-
B) Se2-
C) Rb+
D) Ba2+
E) none of the above


52) Which one of the following species has the electron configuration of 1s22s22p6?
1. Na+
2. O2-
3. F-
A) 1 and 2 only
B) 1 and 3 only
C) 2 and 3 only
D) All of 1, 2, and 3
E) Neither 1, 2, or 3


53) If the electron configuration of a ground state potassium atom is 1s22s22p63s1, the electron configuration of the potassium cation (K+) would be:
A) 1s22s22p63s2
B) 1s22s22p6
C) 1s22s22p63s1
D) 1s12s22p63s1
E) none of the above

54) Choose the answer that best completes the following statement: When an aluminum atom reacts so as to attain a noble gas electron configuration,
A) the atom gains five electrons.
B) the result is a configuration of 1s22s22p6.
C) a 3- ion forms.
D) the noble gas configuration of argon is achieved.
E) none of the above

55) The size of an atom generally increases:
A) down a group and from right to left across a period.
B) up a group and from left to right across a period.
C) down a group and from left to right across a period.
D) up a group and from right to left across a period.
E) up a group and diagonally across the Periodic Table.


56) Which of the following elements has the lowest ionization energy?
A) Rb
B) Na
C) C
D) F
E) He


57) Which of the following elements has the highest ionization energy?
A) Ba
B) Ca
C) Al
D) Cl
E) Ne

58) Which of the following atoms is the largest?
A) Li
B) Na
C) K
D) Rb
E) Cs

59) Which of the following atoms is the smallest?
A) Li
B) Be
C) B
D) O
E) Ne


60) Which of the following atoms has the least metallic character?
A) Li
B) Na
C) K
D) Rb
E) Cs


61) Which of the following atoms has the greatest metallic character?
A) Cs
B) Be
C) Cu
D) Ti
E) Au