Chemistry Quiz on Atomic Structure and Bonding

<p>Chlorine (Cl) (B)</p> Signup and view all the answers

<p>Calcium (Ca) (C)</p> Signup and view all the answers

<p>[Ar] 4s^2 3d^2 (D)</p> Signup and view all the answers

<p>Atoms of different elements can combine in fixed ratios. (C)</p> Signup and view all the answers

<p>Further experimentation would be required to confirm the conclusions. (D)</p> Signup and view all the answers

<p>Hydrogen bonding (A)</p> Signup and view all the answers

<p>Attraction between polar molecules like HCl (C)</p> Signup and view all the answers

<p>Nonpolar molecules (C)</p> Signup and view all the answers

<p>Covalent bonding (B)</p> Signup and view all the answers

<p>Hydrogen bonding (D)</p> Signup and view all the answers

<p>Covalent Bond (A)</p> Signup and view all the answers

<p>Hydrogen bonding involves hydrogen and electronegative atoms. (D)</p> Signup and view all the answers

<p>Ionic Bond (C)</p> Signup and view all the answers

<p>Calcium and Chlorine (C)</p> Signup and view all the answers

<p>NH₃ (A)</p> Signup and view all the answers

<p>Unequal sharing of electrons (C)</p> Signup and view all the answers

<p>CO₂ (A)</p> Signup and view all the answers

<p>Intramolecular forces hold atoms together in a molecule. (C)</p> Signup and view all the answers

<p>It gains electrons and is reduced. (D)</p> Signup and view all the answers

<p>It shifts the equilibrium toward the products. (A)</p> Signup and view all the answers

<p>It is double the number of moles of mercury (II) oxide reacted. (B)</p> Signup and view all the answers

<p>It represents the efficiency of the reaction. (B)</p> Signup and view all the answers

<p>They lower the activation energy of the reaction. (B)</p> Signup and view all the answers

<p>All of the above. (D)</p> Signup and view all the answers

<p>It increases when it is oxidized. (A)</p> Signup and view all the answers

<p>Higher concentration generally increases the reaction rate. (D)</p> Signup and view all the answers

<p>Metallic properties gradually decrease from left to right. (D)</p> Signup and view all the answers

<p>Group IVA (B)</p> Signup and view all the answers

<p>Elements with high ionization energy also tend to have high electron affinity. (A)</p> Signup and view all the answers

<p>p-block (B)</p> Signup and view all the answers

<p>Atomic number 36 (D)</p> Signup and view all the answers

<p>H2 (D)</p> Signup and view all the answers

<p>2 moles (C)</p> Signup and view all the answers

<p>16 L (B)</p> Signup and view all the answers

<p>20 g (C)</p> Signup and view all the answers

<p>Sulphur dioxide (A)</p> Signup and view all the answers

<p>All atoms of the same element have the same number of protons. (B)</p> Signup and view all the answers

<p>Isotopes have the same number of protons. (C)</p> Signup and view all the answers

<p>10 electrons. (B)</p> Signup and view all the answers

<p>4s fills before 3d. (D)</p> Signup and view all the answers

<p>Electrons and protons only. (D)</p> Signup and view all the answers

<p>It is substantially less than the mass of a proton. (D)</p> Signup and view all the answers

<p>The diameter of an atom is 10,000 times that of its nucleus. (B)</p> Signup and view all the answers

<p>5 orbitals. (A)</p> Signup and view all the answers

<p>68.75 g (D)</p> Signup and view all the answers

<p>87.7% (C)</p> Signup and view all the answers

<p>By dividing the percentage yield by 100 and multiplying by theoretical yield. (D)</p> Signup and view all the answers

<p>Reducing agent (A)</p> Signup and view all the answers

<p>Electrons are transferred between substances, changing their oxidation states. (A)</p> Signup and view all the answers

<p>58 litres (C)</p> Signup and view all the answers

<p>112.0 L (C)</p> Signup and view all the answers

<p>50 g (A)</p> Signup and view all the answers

<p>5.6 L (B)</p> Signup and view all the answers

<p>5 moles (B)</p> Signup and view all the answers

A type of chemical bond where two atoms share one or more pairs of electrons. For example, in a water molecule (H₂O), the oxygen atom shares electrons with each hydrogen atom.

A type of chemical bond formed when one atom gives up one or more electrons to another atom. The resulting ions attract each other due to electrostatic forces. For example, in sodium chloride (NaCl), sodium loses an electron to chlorine, forming Na⁺ and Cl⁻ ions.

A type of covalent bond where both electrons in the shared pair come from the same atom. For example, in the ammonium ion (NH₄+), the nitrogen atom provides both electrons in the bond with a hydrogen atom.

A relatively strong intermolecular force that occurs when a hydrogen atom bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine) is attracted to another electronegative atom in a different molecule.

Interactions between atoms in a molecule. These forces hold atoms together within a molecule.

Interactions between molecules. These forces hold molecules together. Weaker than intramolecular forces.

A molecule with a separation of electrical charge, creating a positive and negative end. This results from uneven sharing of electrons.

A molecule where the electrical charge is evenly distributed. No separation of charge.

In any chemical reaction, the total number of atoms of each element remains the same, regardless of the changes in chemical bonds.

A balanced chemical equation has the same number of atoms of each element on both sides of the equation. It represents the conservation of mass.

A reducing agent loses electrons and gets oxidized. It causes the gain of electrons (reduction) in another species.

A catalyst speeds up a reaction without itself being consumed. It provides an alternate pathway with lower activation energy.

The percentage yield compares the actual amount of product obtained to the theoretical yield. It measures the efficiency of a reaction.

The rate of a reaction is influenced by factors such as temperature, concentration, surface area, and catalysts.

At equilibrium, the forward and reverse reaction rates are equal. This doesn't mean equal concentrations of reactants and products.

The equilibrium constant (K) indicates the relative amounts of reactants and products at equilibrium. It's affected by temperature, not by concentration changes.

A model that described atoms as indivisible particles but later found to be incorrect. This is because it did not account for subatomic particles like protons, neutrons, and electrons.

The relative atomic mass of an element is calculated by averaging the masses of its isotopes, weighted by their natural abundances. It takes into account the different isotopes of an element and their proportions.

Electron configuration describes the arrangement of electrons in different energy levels and sublevels within an atom. It helps understand how elements bond and their chemical properties.

John Dalton's atomic theory is still relevant because it laid the foundation for modern chemistry. It introduced the concept of the atom as the fundamental building block of matter.

Thomson's experiment involved determining the charge-to-mass ratio of electrons. If the experiment couldn't be repeated, his conclusions would be invalidated because the results wouldn't be consistent.

A phenomenon observed with elements placed diagonally to each other in the periodic table. These elements exhibit similar chemical properties due to similar effective nuclear charges and ionic radii. For example, lithium (Li) and magnesium (Mg), or beryllium (Be) and aluminum (Al) show diagonal similarities.

The energy required to remove one electron from the outermost shell of a neutral gaseous atom in its ground electronic state. The higher the ionization energy, the harder it is to remove an electron.

The distance between the nucleus and the outermost electron shell in an atom. The smaller the atomic radius, the closer the outer electrons are to the nucleus.

The tendency of an atom to lose electrons and form positive ions (cations). Metals have a strong metallic character.

Oxygen has a higher electronegativity than nitrogen due to its smaller atomic size and greater effective nuclear charge. This means oxygen attracts electrons more strongly, making it more electronegative.

Temporary attractive forces between nonpolar molecules due to temporary fluctuations in electron distribution.

Attractive forces between polar molecules due to the attraction of opposite partial charges.

Transfer of valence electrons from a metal atom to a nonmetal atom, resulting in oppositely charged ions that attract each other.

The property of an element that describes the amount of energy required to remove an electron from a gaseous atom in its ground state.

The tendency of an atom to gain an electron. It's a measure of how much energy is released when an electron is added to a gaseous atom.

The ability of an atom to attract electrons in a bond. It describes how strongly an atom pulls electrons towards itself in a molecule.

The central part of an atom containing protons and neutrons.

The number of protons in an atom's nucleus.

Atoms of the same element with the same number of protons but different numbers of neutrons.

The outermost energy level of an atom.

Electrons in the valence shell that participate in chemical bonding.

A positively charged particle found in the nucleus of an atom.

A neutral particle found in the nucleus of an atom.

A negatively charged particle that orbits the nucleus of an atom.

The reactant that is completely consumed in a chemical reaction, determining the amount of products formed.

The reactants that are present in excess beyond what is needed to react completely with the limiting reactant.

The amount of product that could theoretically be formed based on the stoichiometry of the balanced chemical equation, assuming complete conversion of the limiting reactant.

The actual amount of product obtained from a chemical reaction, which may be less than the theoretical yield due to factors like incomplete reactions or side reactions.

The ratio of the actual yield of a reaction to the theoretical yield, expressed as a percentage. It indicates the efficiency of a reaction, with a higher percentage indicating a more efficient conversion of reactants to products.

A chemical reaction that involves the transfer of electrons between reactants, resulting in a change in the oxidation states of the participating atoms.

A substance that loses electrons in a redox reaction. Its oxidation state increases.

The number assigned to an atom in a molecule or ion that indicates its hypothetical charge assuming that all bonds were ionic.

The volume of a gas at Standard Temperature and Pressure (STP) is 22.4 liters per mole. This relationship helps convert between moles and volume of a gas at STP.

A balanced chemical equation ensures the number of atoms of each element is equal on both sides. This follows the Law of Conservation of Mass, where mass is neither created nor destroyed in a chemical reaction.

A balanced chemical equation provides the mole ratio between reactants and products. This ratio allows you to calculate the amount of reactant or product involved in a reaction given a certain amount of another substance.

To solve mass-volume problems, use the molar mass of the substance and the molar volume of a gas (22.4 L/mol) to set up a proportion. This proportion relates the mass of one substance to the volume of another.

Decomposition reactions involve breaking down a compound into simpler substances. For example, heating calcium carbonate decomposes it into calcium oxide and carbon dioxide. Use stoichiometry to calculate the amounts of reactants and products.