Chemistry Basics Quiz

Chemistry

• Ions form when electrons move from one atom to another. A positive charge indicates electron loss; a negative charge indicates electron gain.
• Valence electrons are the outermost electrons, loosely bound, and available for bonding.
• The number of valence electrons corresponds to a group number on the periodic table. For groups 13-18, subtract 10 to find the number of valence electrons.
• Atoms prefer to be stable while forming compounds; noble gases are already stable.

Bohr-Rutherford Diagrams

• Write the standard atomic notation.
• Calculate protons, electrons, and neutrons (PEN).
• Draw a nucleus (circle) with protons and neutrons inside.
• Draw an orbital (larger circle) around the nucleus and place electrons inside.
• The first orbital holds a maximum of 2 electrons; subsequent orbitals can hold 8 electrons.
• When drawing ions, ensure they are stable.

Five Special Transition Metals

• Copper (Cu): +2 or +1
• Iron (Fe): +3 or +2
• Lead (Pb): +4 or +2
• Tin (Sn): +4 or +2
• Manganese (Mn): +4 or +2

Compounds

• Ionic compounds are formed between a metal and a non-metal. The metal is positive, and the non-metal is negative.
• Polyatomic compounds are ions made of more than one atom acting as a single unit. They are similar to ionic compounds, but with a polyatomic ion acting as the nonmetal.
• Molecular compounds are formed from two or more non-metals.

Writing Chemical Formulas for Ionic Compounds

• Write the symbols for the elements, with the metal first.
• Write the ionic charge above each symbol.
• Crisscross the numbers (ionic charges) downwards. Delete the signs (positive/negative charges).
• Write the crisscrossed numbers as subscripts. Do not write 1.
• Divide subscripts by the highest common denominator.

Naming Ionic Compounds

• Name the metal first using the periodic table.
• Name the nonmetal second, changing the ending to "ide."
• If the metal is one of the five special transition metals, state its charge with Roman numerals.

Writing Chemical Formulas for Polyatomic Compounds

• Write the symbols for the metal and polyatomic ion, writing the metal first.
• Write the ionic charges above each symbol; place brackets around the polyatomic ion.
• Crisscross the numbers downwards; delete the signs.
• Write the crisscrossed numbers as subscripts. Remove brackets if the subscript outside is 1.
• Divide subscripts by the highest common denominator.

Naming Molecular compounds

• Name the first element, using the name from the periodic table.
• Name the second element, using the "ide" ending.
• Use prefixes to indicate the number of atoms of each element.

The Law of Conservation of Mass

• In a chemical reaction, the total mass of the reactants equals the total mass of the products.

Balancing Chemical Equations

• Make an inventory of atoms on both sides of the equation.
• Multiply chemical formulas by coefficients to balance the number of atoms of each element.
• Never change the chemical formula.
• When you change a coefficient, recalculate the inventory to check if it is balanced.

Types of Reactions

• Synthesis: atoms or elements combine to form a new substance. A + B → AB
• Decomposition: a substance breaks down into simpler substances. AB → A + B
• Single Displacement: one element replaces another element in a compound. Z + AB → ZB + A
• Double Displacement: elements in two different compounds exchange places. AB + XY → AY + XB
• Combustion: a substance reacts with oxygen and releases energy, typically oxygen.

Exothermic and Endothermic Reactions

• Exothermic: releases energy (heat or light).
• Endothermic: absorbs energy (heat or light).

Acids and Bases

• Acids: sour taste; corrosive; good conductors; chemically reactive; contain H⁺ ions.
• Bases: bitter taste; corrosive; good conductors; slippery texture; contain OH⁻ ions.

pH Scale

• pH measures the strength of acids and bases.
• A pH of 7 is neutral.
• Lower values are more acidic; higher values are more alkaline.

Optics

Luminosity

• Luminous objects produce their own light.
• Non-luminous objects do not produce their own light.

Sources of Light

• Incandescence: light produced by heat.
• Electric Discharge: light produced by passing an electric current through a gas.
• Phosphorescence: light emitted after absorbing ultraviolet light.
• Fluorescence: immediate emission of visible light after absorbing ultraviolet light.
• Chemiluminescence: light produced by a chemical reaction.
• Bioluminescence: chemiluminescence in living organisms.
• Triboluminescence: light produced when certain crystals are scratched, crushed, or rubbed.

Transparent, Translucent, Opaque

• Transparent: light passes straight through.
• Translucent: some light passes through, but the object is not clear.
• Opaque: no light passes through.

Electromagnetic Spectrum

• Wavelength: distance between two waves.
• Frequency: the number of waves passing a certain point per unit of time.
• Energy: related to the frequency; greater frequency = greater energy.

Plane Mirrors

• Incident ray: incoming ray.
• Reflected ray: ray that bounces.
• Angle of Incidence = Angle of Reflection
• Normal: perpendicular line to the plane of the mirror.

Law of Reflection

• The angle of incidence equals the angle of reflection. The incident ray, reflected ray, and normal all lie in the same plane.

Bending of Light (Refraction)

• Light bends as it enters a medium with a different density.
• Light bends toward the normal when going from a less dense to a more dense medium.
• Light bends away from the normal when going from a more dense to a less dense medium.

Index of Refraction

• The ratio of the speed of light in a vacuum to the speed of light in the medium.
• Index of refraction is calculated using the formula: n=c/v; (Speed of light in a vacuum/Speed of light in the medium)

Biology

Parts of Cells

• Nucleus: Brain of the cell; controls all cellular activities; holds DNA.
• Cell membrane: Flexible double layer that separates the cell’s interior from its surroundings.
• Cytoplasm: fluid-like substance that fills the cell; suspends organelles.
• Mitochondria: Powerhouse of the cell; involved in cellular respiration (producing energy).
• Ribosomes: responsible for protein synthesis
• Endoplasmic Reticulum (ER): network of membranes involved in transporting materials (Rough ER also involved in protein synthesis)
• Vacuoles: fluid-filled structures that store water, food, or waste products.
• Chloroplasts: (plant cells) contains chlorophyll; involved in photosynthesis.
• Cell Wall (plant cells): rigid outer layer that protects and supports the cell.
• Golgi Body: Packages and transports cellular materials.
• Lysosomes: contains digestive enzymes for breaking down waste.

Tissues

• Muscle: responsible for movement (skeletal, smooth, cardiac)
• Epithelial: Covers body surfaces and lines internal organs.
• Connective: Supports and connects other tissue types (blood, bone, cartilage).
• Nervous: transmits electrical signals throughout the body (neurons).

Cell Division (Mitosis)

• Prophase: chromosomes condense, nuclear membrane breaks down, spindle fibers form
• Metaphase: chromosomes line up in the middle of the cell
• Anaphase: sister chromatids separate and move to opposite poles
• Telophase: chromosomes decondense, nuclear membranes reform, spindle fibers break down

Body Systems

• Respiratory System: Breathing
• Circulatory System: Blood circulation
• Digestive System: Digestion and absorption

Gas Exchange

• Gas exchange occurs in the alveoli of the lungs.
• Oxygen diffuses into the blood, and carbon dioxide diffuses out.

Blood Vessels

• Arteries: carry blood away from the heart (thick walls)
• Veins: carry blood back to the heart (thin walls)
• Capillaries: connect arteries and veins, facilitating gas and nutrient exchange.

Cancer

• Benign tumor vs Malignant tumor (how they affect other tissues)
• Treatments for cancer (surgery, radiation, chemotherapy)

Climate Change

• Weather vs Climate (definitions and examples)
• Greenhouse effect (natural process)
• Greenhouse gases (definition, types, most effective/least effective)
• Evidence and impacts of climate change
• Investigating past climates (ice cores, other methods)

Test your knowledge on fundamental principles of chemistry, including ionic and polyatomic compounds, naming conventions, and key concepts like the Law of Conservation of Mass. This quiz reviews essential topics that are crucial for understanding chemical reactions and structures.