An atom is the basic unit of an element and retains its chemical properties. It cannot be subdivided without losing these properties.

Metals are typically malleable, meaning they can be hammered into different shapes. This property differentiates them from most non-metals.

The periodic table is arranged by increasing atomic number, which reveals periodic trends in chemical properties. This method provides a systematic way to predict element behavior.

Electrons carry a negative charge, which is fundamental to understanding atomic structure. This negative charge plays a key role in chemical bonding.

Electrons, especially those in the outer shell, determine how atoms interact and bond with others. Their arrangement directly influences chemical reactivity.

The reaction shows that one carbon atom reacts to produce one molecule of CO2, yielding a molar ratio of 1:1. This straightforward ratio is key to stoichiometric calculations.

By dividing the percentages by the atomic masses (S: 32, O: 16), the mole ratio comes out to approximately 1:3. Hence, the empirical formula is SO3.

Neon has the electron configuration 1s2 2s2 2p6, which means there are 8 electrons in the outer shell. This complete valence shell makes neon chemically inert.

Covalent bonds are formed when atoms share electron pairs. This type of bonding is essential in forming stable molecules.

Exothermic reactions release energy, usually as heat, into the surroundings. This occurs because the energy of the products is lower than that of the reactants.

The law of conservation of mass asserts that mass is neither created nor destroyed in a closed system during a chemical reaction. This principle is fundamental in balancing chemical equations.

The color of reactants does not affect the rate of a chemical reaction. Parameters such as temperature, catalysts, and surface area directly impact reaction rates.

Acids typically have a pH less than 7, while bases have a pH greater than 7. This distinction is crucial for classifying substances as acidic or basic.

In most compounds, oxygen exhibits an oxidation number of -2. This consistency is foundational in understanding redox reactions.

Evaporation is the process in which molecules at the surface of a liquid gain enough energy to become a gas. This phase change occurs gradually under normal conditions.

Calculations show that 10 moles of A can produce 5 moles of C, while 12 moles of B can only yield 4 moles of C based on the stoichiometric ratios. Therefore, B is the limiting reactant, resulting in 4 moles of C.

For an exothermic reaction, increasing the temperature adds heat, causing the equilibrium to shift toward the reactants. This response aligns with Le Chatelier's principle to counteract the added heat.

Methane's central carbon atom forms four equivalent sigma bonds arranged tetrahedrally, which is indicative of sp3 hybridization. This hybridization distributes electron density evenly around the carbon.

The salt bridge enables the movement of ions between the cell's half-cells, maintaining electrical neutrality during the redox process. This prevents charge buildup that would otherwise stop the electrical flow.

Across a period, the number of protons increases, which strengthens the nuclear attraction on the electrons. Since there is minimal additional shielding from electrons, the atomic radius decreases.