Chemistry: Ionic Equations and Moles

<p>It decomposes into CaO and CO2. (D)</p> Signup and view all the answers

<p>1000 (D)</p> Signup and view all the answers

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

<p>To identify spectator ions. (C)</p> Signup and view all the answers

<p>It allows for the calculation of the number of moles present. (C)</p> Signup and view all the answers

<p>K2O (C)</p> Signup and view all the answers

<p>1 mole (A)</p> Signup and view all the answers

<p>Convert mass to moles (A)</p> Signup and view all the answers

<p>Divide each value by the smallest number of moles (D)</p> Signup and view all the answers

<p>CS2 (D)</p> Signup and view all the answers

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

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

<p>Calculating from percentage composition (A)</p> Signup and view all the answers

<p>It contains the same number of atoms of each element on both sides. (B)</p> Signup and view all the answers

<p>Adjust the coefficients in front of the formulae. (C)</p> Signup and view all the answers

<p>Hydrogen peroxide. (B)</p> Signup and view all the answers

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

<p>Peroxide ion (O2^2-) (D)</p> Signup and view all the answers

<p>Adjusting coefficients multiple times during the process. (B)</p> Signup and view all the answers

<p>It would result in a completely different reaction. (A)</p> Signup and view all the answers

<p>Being able to work out chemical formulae accurately. (D)</p> Signup and view all the answers

<p>The anion becomes distorted by the cation's pull. (B)</p> Signup and view all the answers

<p>Inter-molecular forces between molecules. (C)</p> Signup and view all the answers

<p>Ion charge and size influence covalent character in ionic compounds. (D)</p> Signup and view all the answers

<p>Permanent dipole – Permanent dipole attraction. (B)</p> Signup and view all the answers

<p>Size and charge of the ions. (C)</p> Signup and view all the answers

<p>Negative parts of one molecule attract positive parts of another. (D)</p> Signup and view all the answers

<p>Large differences in charge density of ions. (A)</p> Signup and view all the answers

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

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

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

<p>57.14% (C)</p> Signup and view all the answers

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

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

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

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

<p>MgCl2 (C)</p> Signup and view all the answers

<p>They lose their outer electron(s) to become cations. (B)</p> Signup and view all the answers

<p>They hold the metal structure together through electrostatic attraction. (D)</p> Signup and view all the answers

<p>Sea of electrons model. (C)</p> Signup and view all the answers

<p>Cations are surrounded by an electron sea. (B)</p> Signup and view all the answers

<p>Electrons are able to freely move throughout the metal. (A)</p> Signup and view all the answers

<p>Electrons are free to move around positively charged ions. (A)</p> Signup and view all the answers

<p>Metallic bonding includes delocalised electrons instead of localized ones. (C)</p> Signup and view all the answers

<p>High electrical conductivity. (D)</p> Signup and view all the answers

The simplest whole number ratio of atoms in a compound.

A method to determine the empirical formula of a compound by converting the given masses of elements into moles and then simplifying the resulting mole ratio to the simplest whole number ratio.

A method to determine the empirical formula of a compound by converting the given percentage composition of elements into moles and then simplifying the resulting mole ratio to the simplest whole number ratio.

The ratio of atoms in a compound obtained by dividing the number of moles of each element by the smallest number of moles present.

To find the EF of a compound when given the number of moles of each element, first determine the simplest ratio of the elements by dividing by the smallest number of moles.

The number of moles is calculated by dividing the mass of the substance by its molar mass.

The molar mass of a substance is the sum of the atomic masses of all the atoms in its molecular formula.

The mass of one mole of atoms of an element.

The percentage composition by mass of an element in a compound is calculated by dividing the mass of the element by the total mass of the compound and multiplying by 100%.

The empirical formula is the simplest whole number ratio of atoms in a compound. It represents the smallest unit of a compound.

To determine the percentage composition by mass, first calculate the mass of each element in the compound. Then, divide the mass of each element by the total mass of the compound and multiply by 100%.

A chemical equation where the number of atoms of each element is the same on both sides of the reaction arrow.

A set of rules used to ensure that the same number of atoms of each element are present on both sides of a chemical equation. The numbers in front of the formulae (coefficients) can be changed. However, the formulae themselves must remain unchanged.

The numbers written in front of the chemical formula in a balanced chemical equation.

The process of adjusting the coefficients in a chemical equation to ensure the same number of atoms of each element on both sides.

The arrow symbol used in a chemical equation to indicate the direction of the reaction.

The substances undergoing change in a chemical reaction.

The substances formed as a result of a chemical reaction.

A chemical reaction where atoms are re-arranged to form new substances.

The process of separating ionic compounds into their individual ions when dissolved in water, allowing us to analyze their chemical reactions more accurately.

Ions that remain unchanged throughout a reaction and do not participate in the actual chemical change.

An ionic equation where spectator ions have been removed, showing only the species directly involved in the chemical reaction.

A chemical equation written in its full form, including all reactants and products, even spectator ions.

A method for converting moles to mass, volume, or concentration, and vice versa, by using a simple triangular diagram.

The number of moles of a substance present in a given volume of solution.

The ratio of the moles of each reactant and product in a balanced chemical equation.

Unit for volume commonly used in chemistry, equal to 1 cubic decimeter (dm³).

The greater the difference in charge density between the cation and the anion, the more the anion's electron cloud is distorted by the cation's pull.

A type of intermolecular force where the negative end of one polar molecule is attracted to the positive end of another polar molecule.

When the electron cloud of an anion is distorted by a cation's pull, it's called polarization. This often leads to a more covalent character in the overall bond.

An ion's charge density is a measure of the charge of an ion compared to its size. Higher charge density means the charge is concentrated in a smaller space.

The size of the cation and the anion determine the extent of polarization. Smaller ions are more polarizable than larger ones.

The magnitude of the charges on the cation and anion affects polarization. Higher charges lead to greater distortion.

Metallic bonding is a type of chemical bond that occurs between metal atoms. It involves the delocalization of valence electrons, which are free to move throughout the metal lattice. This creates a "sea of electrons" that holds the positively charged metal ions together.

The delocalized electrons in metallic bonding are free to move throughout the metal lattice. This means that they're not fixed to any particular metal atom and can easily carry an electric current.

The ability of metals to be hammered or bent into different shapes without breaking is known as malleability. In metallic bonding, the 'sea of electrons' allows metal atoms to slide past each other without disrupting the overall structure.

Metals are ductile, which means they can be drawn into wires without breaking. This property is also attributed to the 'sea of electrons' in metallic bonding, allowing metal atoms to move past each other while maintaining the overall structure.

Metallic bonding is characterized by the strong electrostatic attraction between the positively charged metal ions and the negatively charged 'sea of electrons'. This strong attraction contributes to the high melting and boiling points of metals.

Delocalized electrons are electrons that are not associated with a specific atom but rather move freely throughout a material. They are responsible for the strong bonding and unique properties of metals, such as good electrical conductivity and malleability.

The "sea of electrons" model describes metallic bonding by visualizing the delocalized electrons as a fluid-like sea that surrounds positively charged metal ions. This model helps explain the unique properties of metals, such as their good conductivity and malleability.

The electrons in metallic bonding are not bound to specific atoms, making metals good conductors of heat. The free-flowing electrons can easily transfer heat energy throughout the metal structure.