Physical Science - Light Elements and Isotopes

<p>Water (H2O) (A)</p> Signup and view all the answers

<p>Water molecules form strong hydrogen bonds with each other. (A)</p> Signup and view all the answers

<p>Boiling point is directly proportional to intermolecular forces. (C)</p> Signup and view all the answers

<p>The relative strength of adhesive forces compared to cohesive forces. (D)</p> Signup and view all the answers

<p>The electronegativity difference between the atoms in the molecule. (C)</p> Signup and view all the answers

<p>Formula Mass is used for compounds with ionic bonds, while Molecular Mass is used for compounds with covalent bonds. (D)</p> Signup and view all the answers

<p>It produces twice as much energy per volume as natural gas. (D)</p> Signup and view all the answers

<p>To relate the number of atoms/molecules to mass. (C)</p> Signup and view all the answers

<p>Decomposition of organic waste in landfills. (C)</p> Signup and view all the answers

<p>An increase in the rate of reaction. (A)</p> Signup and view all the answers

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

<p>Lithium-ion battery (D)</p> Signup and view all the answers

<p>The mass ratios of the elements and the molecular weight of the compound. (D)</p> Signup and view all the answers

<p>To provide an alternate reaction pathway with a lower activation energy. (C)</p> Signup and view all the answers

<p>To facilitate the chemical reaction that releases energy. (D)</p> Signup and view all the answers

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

<p>It has a very high energy density. (C)</p> Signup and view all the answers

<p>Non-renewable energy sources formed from decayed organic matter over millions of years. (B)</p> Signup and view all the answers

<p>Lead-acid battery (C)</p> Signup and view all the answers

<p>To provide a pathway for electron flow. (C)</p> Signup and view all the answers

<p>It is a catalyst in the same physical state as the reaction it catalyzes. (D)</p> Signup and view all the answers

<p>Change the mass in grams of the given substance to moles using its molar mass. (B)</p> Signup and view all the answers

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

<p>By dividing the actual yield by the theoretical yield and multiplying by 100% (A)</p> Signup and view all the answers

<p>The coefficients from the balanced equation. (D)</p> Signup and view all the answers

<p>The amount of product that is produced as a result of the reaction. (B)</p> Signup and view all the answers

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

<p>Number of Neutrons (A)</p> Signup and view all the answers

<p>Supernova Nucleosynthesis (C)</p> Signup and view all the answers

<p>Undergoes radioactive decay (B)</p> Signup and view all the answers

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

<p>Empedocles believed in four fundamental substances, while Democritus proposed the existence of indivisible atoms. (D)</p> Signup and view all the answers

<p>Alchemy incorporated Aristotle's four elements into its system of transforming matter. (B)</p> Signup and view all the answers

<p>Atoms can be broken down into smaller subatomic particles. (C)</p> Signup and view all the answers

<p>Law of Multiple Proportions (A)</p> Signup and view all the answers

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

<p>James Chadwick (B)</p> Signup and view all the answers

<p>It is produced artificially. (D)</p> Signup and view all the answers

<p>The stability of the nucleus (B)</p> Signup and view all the answers

<p>Alpha Decay emits helium nuclei, Beta Decay emits electrons. (A)</p> Signup and view all the answers

<p>Electrons have a definite path around the nucleus. (A)</p> Signup and view all the answers

<p>J.J. Thomson (D)</p> Signup and view all the answers

A method to find moles of substances in a reaction using balanced equation coefficients.

Converting moles to grams or vice versa using the molar mass of a compound.

The reactant that limits the amount of product formed as it gets fully consumed.

The expected amount of product formed from a reaction based on calculations.

The ratio of actual yield to theoretical yield expressed as a percentage.

The process where light elements like Hydrogen and Helium were formed shortly after the Big Bang.

Formation of heavy elements by fusion of lighter nuclei in stars.

Creation of new elements during the explosive death of a star.

When a nucleus captures a neutron to form heavier elements than iron.

A form of an element with the same atomic number but a different mass number.

An isotope that is not radioactive and does not decay.

A radioactive isotope that decays and emits particles to form new elements.

The theory proposing that matter is made of indivisible building blocks called atoms.

Concentration, particle size, temperature, and catalysts influence the speed of chemical reactions.

Higher concentration means more particles available for collisions, accelerating reactions.

Smaller particles have greater surface area, leading to more collisions and faster reactions.

Increased temperature leads to more active molecules, resulting in faster reaction rates.

A substance that accelerates a reaction by lowering the activation energy needed for collisions.

A catalyst in a different physical state from the reactants it helps.

A catalyst that exists in the same physical state as the reactants it catalyzes.

Combustible geologic deposits formed from decayed organic material, formed through heat and pressure.

The ability of an atom to attract electrons; increases left to right and decreases top to bottom.

Molecules with equal electronegativity, sharing electrons equally.

Molecules with uneven electron sharing, creating slight positive and negative ends.

A scale measuring electronegativity; fluorine has the highest value of 4.0.

Determined by the electronegativity difference between bonded atoms.

Attraction between an ion and a polar molecule.

A strong type of dipole-dipole interaction involving hydrogen and electronegative atoms (N, O, F).

Energy needed to increase the surface area of a liquid; linked to intermolecular forces.

Matter is composed of tiny, indivisible particles called atoms.

The total mass in a chemical reaction remains constant, as stated by Antoine Lavoisier in 1789.

If a compound is broken down, the masses of the elements are in the same ratio, as described by Joseph Proust in 1799.

When two elements form different compounds, the mass ratios of one element can be expressed in small whole numbers, according to John Dalton.

Proposed by J.J. Thomson, this model suggests that an atom is a mix of positively-charged 'pudding' with negatively-charged electrons.

Conducted by Ernest Rutherford, showed that atoms have a small, dense positively-charged nucleus containing protons.

The smallest discrete unit of energy, often discussed in the context of atomic structure and behavior.

Elements with atomic numbers 99-118, which are radioactive and artificially created.

A rechargeable battery used in devices like laptops and phones.

A battery with nickel hydroxide and cadmium electrodes, using potassium hydroxide as the electrolyte.

Standard batteries with zinc and carbon electrodes, common in AA, C, and D cells.

Devices converting sunlight into electricity, also called photovoltaic cells.

Organic materials, often considered waste, that can be used for energy.

The measurement of reactants and products in chemical reactions based on quantitative laws.

A counting unit in chemistry, equating to Avogadro's number, 6.02x10^23.

The simplest ratio of elements in a compound derived from mass relations.