Nursing Elites

1. Al(NO3)3 + H2SO4 → Al2(SO4)3 + HNO3 is an example of which kind of reaction?

• A. Decomposition reaction
• B. Synthesis reaction
• C. Single replacement reaction
• D. Double replacement reaction

Correct answer: C

Rationale: The given chemical equation represents a single replacement reaction. In this reaction, aluminum (Al) displaces hydrogen in sulfuric acid (H2SO4), forming aluminum sulfate (Al2(SO4)3) and releasing nitric acid (HNO3). Single replacement reactions involve an element replacing another element in a compound, which is evident in this reaction. Choice A, Decomposition reaction, is incorrect because decomposition reactions involve a single compound breaking down into two or more substances. Choice B, Synthesis reaction, is incorrect as it involves the combination of two or more substances to form a more complex compound. Choice D, Double replacement reaction, is also incorrect as it involves an exchange of ions between two compounds to form two new compounds.

2. What are the 3 types of radiation in nuclear chemistry?

• A. Alpha, Beta, Delta
• B. Alpha, Beta, Gamma
• C. Gamma, Beta, Delta
• D. Delta, Beta, Gamma

Correct answer: B

Rationale: The correct answer is B: Alpha, Beta, Gamma. In nuclear chemistry, the 3 types of radiation are alpha, beta, and gamma radiation. Alpha radiation consists of helium nuclei, beta radiation involves electrons or positrons, and gamma radiation is electromagnetic radiation of high frequency. Choice A is incorrect because 'Delta' is not a type of radiation in nuclear chemistry. Choice C is incorrect as it does not list alpha radiation. Choice D is incorrect as it lists the types in the wrong order and includes 'Delta' instead of alpha radiation.

3. If oxygen is in a compound, what would its oxidation number be?

• A. 2
• B. -2
• C. 0
• D. -1

Correct answer: B

Rationale: Oxygen typically has an oxidation number of -2 in compounds because it tends to gain electrons. This is due to its high electronegativity, which leads to oxygen attracting electrons towards itself in a chemical bond. Choice A (2) is incorrect because oxygen doesn't have a +2 oxidation number in compounds. Choice C (0) is incorrect as oxygen rarely has an oxidation number of 0 in compounds. Choice D (-1) is incorrect as oxygen's oxidation number in compounds is typically -2, not -1.

4. What is the net charge of an ionic compound?

• A. 0
• B. -1
• C. +1
• D. Variable

Correct answer: A

Rationale: The correct answer is A: 0. Ionic compounds have a net charge of 0 because they are formed by the combination of positively charged ions (cations) and negatively charged ions (anions) in a way that neutralizes their charges. This balanced combination results in an electrically neutral compound. Therefore, the net charge of an ionic compound is typically 0. Choices B, C, and D are incorrect because ionic compounds are designed to have a total neutral charge, with the positive charges balancing out the negative charges.

5. What is the oxidation state of the sulfur atom in sulfuric acid H2SO4?

• A. 4
• B. 6
• C. 8
• D. 10

Correct answer: B

Rationale: In sulfuric acid (H2SO4), sulfur has an oxidation state of +6. The oxidation state is determined by considering the overall charge of the compound and the known oxidation states of other elements. In this case, hydrogen is typically +1, and oxygen is -2. To balance the charges and match the compound's overall charge of 0, sulfur must have an oxidation state of +6. Choice A (4) is incorrect because it doesn't balance the charges in the compound. Choices C (8) and D (10) are also incorrect as they are not valid oxidation states for sulfur in this compound.

Similar Questions