States of Matter Overview

<p>Produces an impure product (D)</p> Signup and view all the answers

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

<p>CH2O (B)</p> Signup and view all the answers

<p>CH2O (C)</p> Signup and view all the answers

<p>80% (A)</p> Signup and view all the answers

<p>0.125 M (A)</p> Signup and view all the answers

<p>146.1 g (A)</p> Signup and view all the answers

<p>24 dm3 (D)</p> Signup and view all the answers

<p>2HCl + Na2CO3 -&gt; 2NaCl + H2O + CO2 (B)</p> Signup and view all the answers

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

<p>Increasing the conductivity of electrical wires (C)</p> Signup and view all the answers

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

<p>The products have less energy than the reactants (B)</p> Signup and view all the answers

<p>Determines the amount of product formed (B)</p> Signup and view all the answers

<p>Volume of the reaction vessel (C)</p> Signup and view all the answers

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

<p>Electrolysis requires a molten or aqueous solution of an ionic compound (C)</p> Signup and view all the answers

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

<p>Gases have weak forces between particles and do not have fixed positions. (B)</p> Signup and view all the answers

<p>It is a passive process that occurs naturally. (A)</p> Signup and view all the answers

<p>Contains two or more elements chemically combined. (D)</p> Signup and view all the answers

<p>The number of protons found in an atom. (C)</p> Signup and view all the answers

<p>Group 0 (B)</p> Signup and view all the answers

<p>Particles vibrate more than in solids and have no fixed positions. (A)</p> Signup and view all the answers

<p>It decreases as the particles with the highest kinetic energy evaporate first. (C)</p> Signup and view all the answers

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

<p>React the reactants to form a solution (B)</p> Signup and view all the answers

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

<p>High melting and boiling points (A)</p> Signup and view all the answers

<p>They are mixtures that often exhibit increased hardness. (C)</p> Signup and view all the answers

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

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

<p>Electrolysis of aluminum oxide (D)</p> Signup and view all the answers

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

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

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

<p>They can decrease the yield of the desired product. (D)</p> Signup and view all the answers

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

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

<p>Incorrect stirring methods (C)</p> Signup and view all the answers

<p>Bromine (Br2) (B)</p> Signup and view all the answers

<p>Using the formula q = m c ΔT (C)</p> Signup and view all the answers

<p>Energy is absorbed from the surroundings. (D)</p> Signup and view all the answers

<p>Difference between bonds broken and bonds formed (B)</p> Signup and view all the answers

<p>Nature of the products (C)</p> Signup and view all the answers

<p>The position shifts to favor the reactants. (C)</p> Signup and view all the answers

<p>It favors the production of ammonia. (D)</p> Signup and view all the answers

<p>Oxidation is the loss of electrons; reduction is the gain. (A)</p> Signup and view all the answers

<p>Oxygen always has an oxidation state of -2. (D)</p> Signup and view all the answers

<p>Strong acids fully dissociate in solution. (D)</p> Signup and view all the answers

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

<p>Atoms of the same element with the same number of protons but different numbers of neutrons. (B)</p> Signup and view all the answers

<p>Chlorine gains one electron to become Cl−. (B), Sodium loses one electron to become Na+. (C)</p> Signup and view all the answers

<p>Weak intermolecular forces and do not conduct electricity. (C)</p> Signup and view all the answers

<p>List elements present on both sides. (A)</p> Signup and view all the answers

<p>It loses two electrons. (B)</p> Signup and view all the answers

<p>The average mass of an atom compared to carbon-12. (B)</p> Signup and view all the answers

<p>Moles = Mass / Relative Atomic Mass. (C)</p> Signup and view all the answers

<p>It represents the simplest whole-number ratio of atoms. (D)</p> Signup and view all the answers

<p>Giant ionic structures. (C)</p> Signup and view all the answers

<p>Add 40, 12, and 48 (from three oxygen). (C)</p> Signup and view all the answers

<p>Double covalent bond. (A)</p> Signup and view all the answers

<p>Each aluminium loses three electrons to oxygen. (B)</p> Signup and view all the answers

<p>Weak intermolecular forces. (B)</p> Signup and view all the answers

<p>They have strong covalent bonds throughout. (B)</p> Signup and view all the answers

<p>High electrical energy requirements (B)</p> Signup and view all the answers

<p>It is treated to be clean and drinkable. (B)</p> Signup and view all the answers

<p>Needed for root growth and ripening. (D)</p> Signup and view all the answers

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

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

<p>Increased levels of greenhouse gases due to human activities (C)</p> Signup and view all the answers

<p>Increasing fossil fuel usage (B)</p> Signup and view all the answers

<p>Formation of acid rain (D)</p> Signup and view all the answers

<p>They follow the general formula CnH2n+2. (D)</p> Signup and view all the answers

<p>They follow the general formula CnH2n. (B)</p> Signup and view all the answers

<p>It dictates the chemical properties of a compound. (A)</p> Signup and view all the answers

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

<p>Breaks down large hydrocarbons into smaller ones. (D)</p> Signup and view all the answers

<p>The bromine water changes from orange to colorless. (A)</p> Signup and view all the answers

Different forms in which matter can exist: solid, liquid, gas.

The process of changing from solid to liquid due to heat.

Process where particles with high energy escape from liquid to gas.

Movement of particles from high concentration to low concentration.

The smallest unit of a substance that can exist independently.

A pure substance made of only one type of atom.

A substance formed from two or more elements chemically combined.

Group 0 elements in the periodic table with full outer electron shells.

Alcohols can be oxidized by burning, microbes, or potassium dichromate.

A method of making alcohol using sugars and yeast.

Reacting ethene with water to produce alcohol.

Acids containing a carboxyl (COOH) group.

Methanoic, Ethanoic, Propanoic are the first three carboxylic acids.

Atoms of the same element with differing neutrons.

Charged particles formed by gaining or losing electrons.

Atoms share electrons to achieve full outer shells.

Electrons are transferred from one atom to another, forming ions.

Adjust coefficients to equalize atom counts on both sides.

Ratio of average mass of an atom compared to carbon-12.

Moles = Mass / Relative Atomic Mass.

Arrangements of atoms in molecules; giant to simple.

Empirical shows simplest ratio, while molecular shows actual count.

Common ions include NH4+, CO32-, SO42-, and NO3-.

Strong bonds throughout with high melting points.

Weak forces with low melting points. Do not conduct electricity.

Sum of atomic masses of all atoms in a molecule.

Sodium loses one electron to become Na+, chlorine gains to become Cl-.

Represents actual number of atoms of each element in a compound.

Shows the simplest ratio of elements in a compound.

List elements, set up a table, find moles, simplify ratios.

Use balanced equations for mole ratios of reactants/products.

The reactant that remains after a reaction is complete.

Calculate how much product was actually made vs. theoretically possible.

Used for neutralization reactions to determine concentrations.

The number of atoms/molecules in one mole of a substance (6.02 x 10²³).

Process using electricity to drive a chemical reaction.

Coating an object with a thin layer of another metal.

Devices converting hydrogen and oxygen into energy with water as a byproduct.

Reactions that release heat energy.

Reactions that absorb heat energy.

Calculate gas volumes based on moles at standard conditions.

Calculate mass of water using the difference from anhydrous compound.

Guidelines to determine the solubility of salts in water, highlighting exceptions.

Method used to obtain soluble salts from a solution by cooling and evaporation.

Technique to create insoluble salts by reacting two soluble salts.

Highly reactive metals in Group 1 of the periodic table, stored in oil.

List of metals arranged by their decreasing reactivity, from potassium to gold.

Group 7 elements that become less reactive as you descend the group.

Characteristics like high melting points, conductivity, and malleability.

Characteristics including dullness, low melting points, and brittleness.

Due to its low density and conductivity, it's ideal for airplanes and cooking.

Excellent conductor used in electrical wiring and cooking vessels.

Process of obtaining iron from ore using a blast furnace.

Methods to prevent iron corrosion including painting and galvanizing.

Electrolytic method used to extract aluminium due to its high reactivity.

Involves reacting specific acids with metal oxides or carbonates.

An alloy of iron, chromium, and nickel, known for corrosion resistance.

The minimum energy needed for a reaction to occur.

Substances that lower activation energy, providing an alternate pathway for reactions.

The heat content change during a chemical reaction, measured in experiments.

Molecules consisting of two atoms, including H2, N2, O2, etc.

Energy required to break bonds, used to calculate enthalpy change.

Temperature, concentration, and surface area affect reaction rate.

Rates can be assessed via changes in volume or concentration over time.

State where forward and reverse reaction rates are equal, resulting in no overall change.

Industrial synthesis of ammonia from nitrogen and hydrogen; exothermic reaction.

Loss of electrons during a chemical reaction.

Gain of electrons during a chemical reaction.

Acids donate H+, while bases accept H+ or produce OH-.

Salts form when hydrogen ions in acids are replaced by metals or ammonium.

Pure water boils at 100°C under standard conditions.

A chemical that turns blue when it comes in contact with water.

Water that is clean and safe to drink.

Essential nutrients include nitrogen, phosphorus, and potassium.

Air is 78% nitrogen, 21% oxygen, and less than 1% other gases.

It's the trapping of heat by greenhouse gases in Earth's atmosphere.

Rain becomes acidic from oxides of sulfur and nitrogen.

Process by which plants make food using sunlight, CO2, and water.

Saturated hydrocarbons with single bonds (CnH2n+2).

Unsaturated hydrocarbons with at least one double bond (CnH2n).

A group of compounds with a similar structure and properties.

Part of a compound responsible for its chemical properties.

Separation technique that sorts hydrocarbons by boiling points.

Breaking down large hydrocarbons into smaller, valuable ones.

Organic compounds featuring a hydroxyl (OH) group.