Question 1

Which of the following pairs of atoms, specified in terms of subatomic particle composition, are isotopes?
A) (24p, 24e, 24n) and (25p, 25e, 25n)
B) (24p, 24e, 24n) and (24p, 24e, 28n)
C) (24p, 24e, 28n) and (25p, 25e, 28n)
D) more than one correct response
E) no correct response

Accepted Answer

Isotopes have the same number of protons but different numbers of neutrons. Pair A and C have different numbers of protons and pair B has the same number of protons (24) but a different number of neutrons (24 in the first atom and 28 in the second atom). Therefore, pair B is the only pair that represents isotopes.

Question 2

Which of the following statements is correct for 
A) atomic number = 27 and mass number = 14
B) contains 14 protons and 27 neutrons
C) contains an equal number of protons and electrons
D) more than one correct response
E) no correct response

Accepted Answer

The answer of Which of the following statements is correct...

Question 3

Element A exists in three isotopic forms with masses of 21.0, 25.0 and 26.0 amu, respectively. Element Q also exists in three isotopic forms with masses of 20, 24.0 and 25.0 amu, respectively. It is true that:
A) Element A has a lower atomic mass than element Q since it has the lightest isotope.
B) Elements A and Q have identical atomic masses since the sums of their isotopic masses are equal.
C) Element Q has a higher atomic mass than element A since its atomic masses are closer together.
D) More than one correct response.
E) No correct response.

Accepted Answer

The average atomic mass of an element depends on both the masses and the relative abundances of its isotopes, not just the sum of the isotopic masses or the mass of the lightest isotope. Since information about the relative abundances of the isotopes is not provided, none of the statements can be determined to be true.

Question 4

Which of the following statements concerning the nucleus of an atom is correct?
A) It accounts for almost all of the mass of an atom.
B) It is always positively charged.
C) It contains only neutrons.
D) More than one correct response.
E) No correct response.

Accepted Answer

The nucleus of an atom accounts for almost all of the mass of an atom due to the presence of protons and neutrons, both of which have significantly more mass than electrons. It is always positively charged because it contains protons, which have a positive charge.

Question 5

Which of the following characterizations for the element ₅₂Te is correct? A) both a representative element and a metal B) electron configuration involves a partially filled s subshell C) electron configuration involves a total of 52 electrons D) more than one correct response E) no correct response

Accepted Answer

Tellurium (Te) has an atomic number of 52, meaning it has 52 electrons in its electron configuration.

Question 6

Characterize EACH of the following statements as being TRUE or FALSE and then indicate the collective true-false status using the choices provided. (1) The shape of an s orbital is always spherical.
(2) All naturally occurring atoms of an element must be identical to each other in terms of subatomic particle makeup.
(3) The alkaline earth metals are the elements in group IA of the periodic table.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Accepted Answer

1) True - s orbitals are always spherical in shape. 2) False - Isotopes of an element have different numbers of neutrons, so not all atoms of an element are identical in subatomic particle makeup. 3) False - The alkaline earth metals are in group IIA, not group IA (which contains the alkali metals).

Question 7

Characterize EACH of the following statements as being TRUE or FALSE and then indicate the collective true-false status using the choices provided. (1) Electrons occupy the orbitals of a subshell such that each orbital acquires one electron before any orbital acquires a second electron.
(2) The nucleus of an atom is always positively charged.
(3) Both electrons and protons are massive particles when compared with neutrons.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Accepted Answer

(1) False - The statement is referring to Hund's rule, which is only true for atoms in their ground state. However, if an atom is in an excited state, some orbitals may have more than one electron before all orbitals have one electron. 
(2) True - The nucleus of an atom is always positively charged, as it contains positively charged protons.
(3) False - Neutrons are actually slightly more massive than both electrons and protons.

Question 8

Characterize EACH of the following statements as being TRUE or FALSE and then indicate the collective true-false status using the choices provided. (1) The number of elements that are metals and nonmetals is approximately equal.
(2) The number of orbitals present in an electron subshell is always six.
(3) An atom as a whole is electrically neutral because all charged subatomic particles reside in the nucleus.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Accepted Answer

1) False - The periodic table contains more metals than nonmetals. 2) False - The number of orbitals in a subshell depends on the type of subshell (s, p, d, f), not always six. 3) False - An atom is electrically neutral because the number of protons (positive charge) in the nucleus equals the number of electrons (negative charge) surrounding the nucleus, not because all charged particles are in the nucleus.

Question 9

Period number and group number in the periodic table are numerically equal for which of the following elements? A) (₁₃Al) B) (₃₃As) C) (₅₁Sb) D) more than one correct response E) no correct response

Accepted Answer

Elements in the periodic table that have their period number and group number numerically equal are typically found in the main groups (s and p blocks). Aluminum (Al) with atomic number 13 is in period 3 and group 13, and Arsenic (As) with atomic number 33 is in period 4 and group 15, not matching the criteria. However, Antimony (Sb) with atomic number 51 is not in a period and group that are numerically equal. The correct interpretation here is that both Aluminum (Al) and Arsenic (As) are incorrectly analyzed in the explanation, leading to a misunderstanding. The correct statement should acknowledge that only Aluminum (Al) fits the criteria of having its period number and group number numerically equal, being in period 3 and group 13. Therefore, the initial response indicating more than one correct response was incorrect, and the accurate answer should be that only Aluminum (Al) fits the described criteria, making the correct choice "A" for Aluminum.

Question 10

Which of the following collections of subatomic particles possesses a net charge of +2?
A) two neutrons and two electrons
B) three protons and one electron
C) three electrons and one proton
D) more than one correct response
E) no correct response

Accepted Answer

Three protons (+3) and one electron (-1) gives a net charge of +2. A is incorrect because neutrons have no charge, while electrons have a negative charge. C is incorrect because electrons have a negative charge while protons have a positive charge. D is incorrect because there is only one correct response. E is incorrect because there is a correct response.

Question 11

Which of the following periodic table groups contains three or more nonmetallic elements?
A) IIIA
B) IVA
C) VA
D) more than one correct response
E) no correct response

Accepted Answer

Group VA (pronounced "group five A") contains nitrogen, phosphorus, arsenic, antimony, and bismuth. Nitrogen and phosphorus are nonmetals, while arsenic and antimony have both metallic and nonmetallic properties, and bismuth is a metal. Therefore, there are at least three nonmetallic elements in this group.

Question 12

Which of the following statements concerning types of elements is correct?
A) There are more noble gas elements than transition elements.
B) There are more s-block elements than d-block elements.
C) There are more nonmetals than metals.
D) More than one correct response.
E) No correct response.

Accepted Answer

The answer of Which of the following statements concerning types...

Question 13

Characterize EACH of the following statements as being TRUE or FALSE and then indicate the collective true-false status using the choices provided. (1) The mass of an atom and the mass of its nucleus are essentially the same.
(2) Two of the six electrons present in an atom of carbon are unpaired.
(3) The element aluminum is located in the d area of the periodic table.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Accepted Answer

(1) False - The mass of an atom includes the mass of its nucleus and the mass of its electrons. Since the electrons have such a small mass compared to the nucleus, the mass of an atom is dominated by the mass of its nucleus. 
(2) True - Carbon has four valence electrons, of which two are unpaired. 
(3) False - Aluminum is located in the p area of the periodic table.

Question 14

Two unpaired electrons are present in the orbital diagram of which of the following elements? A) (₆C) B) (₁₀Ne) C) (₁₂Mg) D) more than one correct response E) no correct response

Accepted Answer

Carbon (C) has an atomic number of 6, with an electron configuration of 1s² 2s² 2p². The two electrons in the 2p orbital are unpaired.

Question 15

Which of the following statements correctly describes the subatomic particle called a neutron?
A) has a mass slightly less than that of a proton
B) is not found in the nucleus
C) has a positive charge
D) more than one correct response
E) no correct response

Accepted Answer

Neutrons have a mass slightly more than that of a proton, are found in the nucleus, and have no charge.

Question 16

Which of the following electron configurations corresponds to an element in the same group of the periodic table as the element whose electron configuration is 1s²2s²2p⁵? A) 1s²2s²2p⁴ B) 1s²2s²2p⁶ C) 1s²2s²2p⁶3s²3p⁶4s²3d⁵ D) more than one correct response E) no correct response

Accepted Answer

The given electron configuration does not correspond to any real element's electron configuration due to the use of non-standard notation and symbols, making it impossible to accurately determine the group of the periodic table it belongs to or match it with any of the provided options.

Question 17

Which of the following characterizations for the element ₂₃V is correct? A) a period 4 element B) electron configuration ends in d³ C) an inner-transition element D) more than one correct response E) no correct response

Accepted Answer

- ₂₃V has 23 total electrons, which corresponds to a period 3 element. - The electron configuration ends in d³, which is incorrect because d-orbitals are not present in the ground state electron configuration of any element in period 3. - ₂₃V cannot be an inner-transition element because its electron configuration does not have any partially filled f-orbitals. Therefore, D is the best choice because there is more than one incorrect statement about the element.

Question 18

Both a number and a letter are used in designating an electron subshell. The letter
A) indicates the shell to which the subshell belongs
B) may be s, p, d, or f
C) gives information about the maximum number of electrons the subshell can contain
D) more than one correct response
E) no correct response

Accepted Answer

The letter used in designating an electron subshell can be s, p, d, or f and it indicates the shape of the subshell. The number used in designating an electron subshell indicates the shell to which the subshell belongs and gives information about the maximum number of electrons the subshell can contain. Therefore, both a letter and a number are necessary to fully designate an electron subshell.

Question 19

Tin is element number 50. This means that all tin atoms have
A) an atomic number of 50
B) 50 neutrons in the nucleus
C) a total of 50 subatomic particles in the nucleus
D) more than one correct response
E) no correct response

Accepted Answer

The atomic number represents the number of protons in an atom's nucleus. Since tin is element number 50, all tin atoms have 50 protons in their nucleus, which corresponds to their atomic number.

Question 20

Characterize EACH of the following statements as being TRUE or FALSE and then indicate the collective true-false status using the choices provided. (1) The sum of the mass number and the atomic number for an atom corresponds to the total number of subatomic particles present in the atom. (2) The element sulfur is both a nonmetal and a representative element. (3) Elements with electron configurations that end in p⁴ would be found in group VIA of the periodic table. A) All three statements are true. B) Two of the three statements are true. C) Only one of the statements is true. D) None of the statements is true.

Accepted Answer

The answer of Characterize EACH of the following statements as...

Quiz 3: Atomic Structure and the Periodic Table

Which of the following pairs of atoms, specified in terms of subatomic particle composition, are isotopes?

Which of the following statements is correct for

Element A exists in three isotopic forms with masses of 21.0, 25.0 and 26.0 amu, respectively. Element Q also exists in three isotopic forms with masses of 20, 24.0 and 25.0 amu, respectively. It is true that:

Which of the following statements concerning the nucleus of an atom is correct?

Which of the following characterizations for the element 52Te is correct?

Period number and group number in the periodic table are numerically equal for which of the following elements?

Which of the following collections of subatomic particles possesses a net charge of +2?

Which of the following periodic table groups contains three or more nonmetallic elements?

Which of the following statements concerning types of elements is correct?

Two unpaired electrons are present in the orbital diagram of which of the following elements?

Which of the following statements correctly describes the subatomic particle called a neutron?

Which of the following electron configurations corresponds to an element in the same group of the periodic table as the element whose electron configuration is 1s22s22p5?

Which of the following characterizations for the element 23V is correct?

Both a number and a letter are used in designating an electron subshell. The letter

Tin is element number 50. This means that all tin atoms have

Which of the following characterizations for the element ₅₂Te is correct?

Which of the following electron configurations corresponds to an element in the same group of the periodic table as the element whose electron configuration is 1s²2s²2p⁵?

Which of the following characterizations for the element ₂₃V is correct?