CHEM 101 (E-1) Chemistry I - Ramsey Exam 2 - Eastwick College
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Free CHEM 101 (E-1) Chemistry I - Ramsey Exam 2 - Eastwick College Questions
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hydrogen
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fluorine
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chlorine
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neon
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helium
Explanation
Fluorine has the highest electronegativity of all elements on the periodic table, with a value of approximately 3.98 on the Pauling scale. Its position at the top right of the periodic table (excluding noble gases), combined with its small atomic radius and strong nuclear charge, gives it an exceptionally strong ability to attract bonding electrons toward itself.
Why the other options are incorrect:
A. Hydrogen Hydrogen has a relatively low electronegativity of approximately 2.20, far below fluorine's value.
C. Chlorine Chlorine is the second most electronegative nonmetal commonly encountered in chemistry, with an electronegativity of approximately 3.16, but it is still lower than fluorine's.
D. Neon Noble gases like neon do not have a defined Pauling electronegativity because they do not typically form chemical bonds, making them irrelevant to the electronegativity scale in the conventional sense.
E. Helium Like neon, helium is a noble gas that does not form bonds under normal conditions and does not have a meaningful Pauling electronegativity value.
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208 amu
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386 amu
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224 amu
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180 amu
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194 amu
Explanation
The formula mass of cholesterol is calculated by summing the atomic masses of all atoms in the molecular formula: 27 carbon atoms (27 × 12.011), 46 hydrogen atoms (46 × 1.008), and 1 oxygen atom (15.999). Adding these together gives a total formula mass of approximately 386.66 amu, which rounds to 386 amu, confirmed by calculation.
Why the other options are incorrect:
A. 208 amu This value is far too low and does not account for the full atomic composition of cholesterol's 27 carbon, 46 hydrogen, and 1 oxygen atoms.
C. 224 amu This value is too low and does not match the correct summation of atomic masses for the complete cholesterol molecular formula.
D. 180 amu This value is significantly too low and likely reflects an incomplete or incorrect calculation of the molecular formula's components.
E. 194 amu This value is also far too low to account for the full mass contribution of all 27 carbon, 46 hydrogen, and 1 oxygen atoms in cholesterol.
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compound
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nucleus
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ion
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mixture
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element
Explanation
Correct Answer: (E) element
An element is a pure substance that cannot be broken down into simpler substances by chemical means. It consists of only one type of atom, making it the simplest and most fundamental form of matter among pure substances. All compounds and mixtures are ultimately composed of combinations of elements.
Why the other options are incorrect:
A. Compound A compound is formed when two or more different elements chemically combine in fixed proportions. It is more complex than an element since it requires multiple types of atoms bonded together.
B. Nucleus The nucleus is the dense central core of an atom containing protons and neutrons. It is a subatomic structure, not a classification of substance.
C. Ion An ion is an electrically charged atom or molecule resulting from the gain or loss of electrons. It is not classified as the simplest form of a substance.
D. Mixture A mixture consists of two or more substances physically combined without a fixed ratio, making it more complex than a single element.
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0
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-18
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-2
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+2
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None of these
Explanation
The charge of an ion is determined by subtracting the number of electrons from the number of protons. With 16 protons and 18 electrons, the calculation is 16 - 18 = -2, indicating that the ion has 2 more electrons than protons, giving it a net charge of -2.
Why the other options are incorrect:
A. 0 A charge of 0 would only occur if the number of protons equaled the number of electrons, which is not the case here since there are 18 electrons and only 16 protons.
B. -18 This value incorrectly uses the total number of electrons as the charge rather than calculating the difference between protons and electrons.
D. +2 A +2 charge would indicate a loss of electrons relative to protons, but this ion has gained electrons (18 electrons compared to 16 protons), making this charge incorrect.
E. None of these This option is incorrect because -2 is indeed a valid and correct answer choice present among the options.
Which of these is the correct formula for aluminum oxide?
- AlO
- Al₃O₂
- Al₂O₃
- Al₂O₂
- AlO₂
Explanation
Explanation:
Correct Answer: (C) Al₂O₃
Aluminum forms a 3+ cation (Al³⁺) and oxygen forms a 2- anion (O²⁻). To write the correct ionic formula, the charges must balance to zero. Using the cross-multiply method: the charge of aluminum (3) becomes the subscript for oxygen, and the charge of oxygen (2) becomes the subscript for aluminum, giving Al₂O₃. Checking: 2 × (+3) = +6 and 3 × (−2) = −6, which sum to zero. The formula is correct and in its simplest form.
Why Other Options are Incorrect:
A. AlO — This implies a 1:1 ratio of Al to O. For charges to balance, Al would need a 2+ charge, but aluminum's stable charge is 3+. This formula does not achieve charge neutrality.
B. Al₃O₂ — This ratio gives a total charge of 3 × (+3) = +9 and 2 × (−2) = −4, which do not balance to zero.
D. Al₂O₂ — This simplifies to AlO (1:1 ratio) and does not correctly balance the 3+ and 2- charges of aluminum and oxide ions.
E. AlO₂ — This would require aluminum to have a 4+ charge to balance two oxide ions (2 × 2− = 4−), but aluminum's stable ionic charge is 3+, not 4+.
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Ag+
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Cd2+
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Pd+
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Ag-
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Pd-
Explanation
Correct Answer: (A) Ag+
The element with 47 protons is silver (Ag), as the atomic number defines the identity of an element. Since the ion has 46 electrons, which is one less than the number of protons (47), it has lost one electron, resulting in a net positive charge of +1. This gives the ion Ag+.
Why the other options are incorrect:
B. Cd2+ Cadmium has an atomic number of 48, not 47, so this does not match the given proton count.
C. Pd+ Palladium has an atomic number of 46, not 47, so this does not match the given proton count.
D. Ag- A negative charge would require more electrons than protons, but this ion has fewer electrons (46) than protons (47), ruling out a negative charge.
E. Pd- Palladium has an atomic number of 46, not 47, and a negative charge would be inconsistent with having fewer electrons than protons.
Which of these statements about an atom is incorrect?
- The mass number minus the atomic number equals the number of neutrons in the atom.
- The number of protons equals the number of electrons.
- The mass number is the sum of protons and neutrons in the atom.
- The number of protons always equals the number of neutrons.
- The number of protons equals the atomic number.
Explanation
Explanation:
Correct Answer: (D) The number of protons always equals the number of neutrons.
This statement is incorrect because protons and neutrons are not always equal in number. While some lighter elements like carbon-12 (6 protons, 6 neutrons) happen to have equal counts, many elements and isotopes have more neutrons than protons. For example, uranium-235 has 92 protons but 143 neutrons. There is no rule requiring proton and neutron counts to be equal.
Why Other Options Are Incorrect:
A. The mass number minus the atomic number equals the number of neutrons — This is a true and standard formula: neutrons = mass number − atomic number.
B. The number of protons equals the number of electrons — This is true for neutral atoms. Protons and electrons are equal in number, giving the atom no net charge.
C. The mass number is the sum of protons and neutrons in the atom — This is the correct definition of mass number and is therefore a true statement.
E. The number of protons equals the atomic number — This is also true and is the very definition of the atomic number.
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NO-
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NO3+
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NO3-
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NO2-
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NO32-
Explanation
The nitrate ion is a polyatomic ion consisting of one nitrogen atom bonded to three oxygen atoms, carrying an overall charge of -1. This is a commonly recognized and standardized polyatomic ion formula used extensively in chemistry, particularly in naming nitrate salts.
Why the other options are incorrect:
A. NO- This formula does not represent the nitrate ion, as it only contains one oxygen atom and does not match the correct composition of nitrate.
B. NO3+ This is incorrect because the nitrate ion carries a negative charge, not a positive charge.
D. NO2- This formula represents the nitrite ion, which contains two oxygen atoms, not three, distinguishing it from nitrate.
E. NO32- This is incorrect because the nitrate ion carries a charge of -1, not -2.
Which of these is not a covalent compound?
- AlCl₃
- C₂H₂
- XeF₄
- TeCl₄
- H₂O
Explanation
Explanation:
Correct Answer: (A) AlCl₃
AlCl₃ (aluminum chloride) is an ionic compound, not a covalent compound. Aluminum is a metal and chlorine is a nonmetal; their combination results in electron transfer from aluminum to chlorine, forming Al³⁺ and Cl⁻ ions held together by electrostatic attraction. Covalent compounds are formed between two nonmetals through electron sharing.
Why Other Options are Incorrect:
B. C₂H₂ — Acetylene is a covalent compound formed between two nonmetals, carbon and hydrogen, sharing electrons through covalent bonds.
C. XeF₄ — Xenon tetrafluoride is a covalent compound. Xenon (a noble gas) and fluorine (a nonmetal) form a covalent compound through electron sharing.
D. TeCl₄ — Tellurium tetrachloride is a covalent compound. Tellurium is a metalloid and chlorine is a nonmetal; their electronegativity difference and bonding properties result in covalent bond formation.
E. H₂O — Water is a classic example of a polar covalent compound, formed by electron sharing between hydrogen and oxygen, both nonmetals.
Which of these does not form a positive ion in an ionic compound?
- P
- Rb
- Ba
- Sn
- Mg
Explanation
Explanation:
Correct Answer: (A) P (Phosphorus)
Phosphorus is a nonmetal. In ionic compounds, nonmetals gain electrons to form negative ions (anions), not positive ions (cations). Therefore, phosphorus does not form a positive ion.
Why Other Options Are Incorrect:
B. Rb (Rubidium) — Rubidium is an alkali metal in Group 1 and readily loses one electron to form Rb⁺, a positive ion.
C. Ba (Barium) — Barium is an alkaline earth metal in Group 2 and loses two electrons to form Ba²⁺, a positive ion.
D. Sn (Tin) — Tin is a metal that forms positive ions, commonly Sn²⁺ or Sn⁴⁺, in ionic compounds.
E. Mg (Magnesium) — Magnesium is an alkaline earth metal that loses two electrons to form Mg²⁺, a positive ion.
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