Free NSAA Chemistry Questions and Answers
Which type of intermolecular force is the strongest?
Hydrogen bonds are the strongest type of intermolecular force compared to London dispersion forces and dipole-dipole interactions.
Which of the following elements has the highest electronegativity?
Fluorine has the highest electronegativity of all elements, meaning it has a strong ability to attract electrons in a chemical bond.
What type of reaction is represented by the following equation: 2H₂ + O₂ → 2H₂O?
The given equation represents a synthesis reaction, where two or more reactants combine to form a single product.
What is the molecular geometry of methane (CH₄)?
Methane (CH₄) has a tetrahedral molecular geometry, with four hydrogen atoms symmetrically distributed around the central carbon atom.
What is the pH of a 0.01 M solution of HCl?
HCl is a strong acid that dissociates completely in water. The pH is calculated as -log[H⁺], so for a 0.01 M solution, pH = -log(0.01) = 2.
What is the oxidation state of manganese in KMnO₄?
In KMnO₄, potassium has an oxidation state of +1 and oxygen has an oxidation state of -2. To balance the charges, manganese must have an oxidation state of +7.
Which of the following statements about catalysts is true?
Catalysts increase the rate of a reaction by lowering the activation energy and are not consumed during the reaction.
Which of the following is the correct electron configuration for a neutral atom of sulfur (atomic number 16)?
The electron configuration for sulfur, which has 16 electrons, is 1s² 2s² 2p⁶ 3s² 3p⁴.
Which of the following compounds is ionic?
Sodium chloride (NaCl) is an ionic compound, consisting of positively charged sodium ions and negatively charged chloride ions.
In the periodic table, which trend is observed as you move from left to right across a period?
As you move from left to right across a period, elements become less metallic and more non-metallic in character.
Which of the following compounds will exhibit hydrogen bonding?
Ammonia (NH₃) exhibits hydrogen bonding due to the presence of a highly electronegative nitrogen atom bonded to hydrogen atoms.
