Physics - Waves and Electromagnetic Spectrum

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Questions and Answers

What is the pH value of a neutral substance?

  • 0
  • 14
  • 3
  • 7 (correct)

How does the distance of valence electrons from the nucleus affect the reactivity of metals?

  • The further the electrons, the less reactive the metal.
  • The distance has no effect on reactivity.
  • The further the electrons, the more reactive the metal. (correct)
  • The closer the electrons, the more reactive the metal.

Acids taste bitter.

False (B)

Non-metals gain electrons to achieve a full outer shell and are less reactive when their valence electrons are further from the nucleus.

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

What is produced when acids react with bases?

<p>Salt and water</p> Signup and view all the answers

What process occurs when an atom loses or gains electrons?

<p>Ionic bonding</p> Signup and view all the answers

The _____ scale ranges from 0 to 14, measuring acidity and alkalinity.

<p>pH</p> Signup and view all the answers

A _ gains electrons and becomes negatively charged.

<p>anion</p> Signup and view all the answers

Which type of radiation can penetrate through air and paper but can be stopped by aluminum?

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

Match the type of bonding with its description:

<p>Ionic Bonding = Atoms lose or gain electrons Covalent Bonding = Atoms share electrons Anion = Negatively charged ion Cation = Positively charged ion</p> Signup and view all the answers

Match the following types of reactions with their corresponding results:

<p>Neutralization = Salt + Water Acid Carbonate = Salt + Water + Carbon Dioxide + Heat Acid Metal = Hydrogen Gas + Salt Chemical Reaction = Change in arrangement of electrons</p> Signup and view all the answers

Which of the following statements about valency is true?

<p>Valency is the number of electrons an atom must gain or lose. (D)</p> Signup and view all the answers

Stable nuclei have too many protons and are radioactive.

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

The law of conservation of mass states that matter can be created or destroyed during a chemical reaction.

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

What is the primary use of gamma rays in medicine?

<p>Nuclear imaging and radiotherapy</p> Signup and view all the answers

Ionic compounds are formed through the bonding of a _ and a _.

<p>cation, anion</p> Signup and view all the answers

Which of the following elements is classified as a non-metal?

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

All atoms become stable by gaining or losing valence electrons.

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

What is the maximum number of electrons that the second shell of an atom can hold?

<p>8</p> Signup and view all the answers

Sodium Chloride is commonly known as ______.

<p>table salt</p> Signup and view all the answers

Match the following groups of the periodic table with their characteristics:

<p>Alkali Metals = Highly reactive, especially with water Alkaline Earth Metals = Reactive but less than alkali metals Noble Gases = Inert gases, do not react easily Halogens = Very reactive non-metals</p> Signup and view all the answers

Which particle in an atom has a positive charge?

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

Electrons are larger than protons and neutrons.

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

What is the process called when an atom emits light after being heated?

<p>Excitation and emission</p> Signup and view all the answers

Flashcards

Electron Shells

Energy levels that electrons orbit the nucleus around.

Reactivity of Metals

Metals react more readily when valence electrons are further away from the nucleus, easier to lose.

Reactivity of Nonmetals

Nonmetals react less readily when valence electrons are further away from the nucleus, harder to gain.

Valency

The number of electrons an atom gains or loses during a chemical reaction.

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Valence Shell

The outermost electron shell of an atom.

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Ionic Bonding

Atoms lose or gain electrons to form ions with opposite charges, attracting each other.

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Covalent Bonding

Atoms share electrons to achieve a full valence shell.

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Anion

A negatively charged ion formed when an atom gains electrons.

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Cation

A positively charged ion formed when an atom loses electrons.

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Ionic Compound

A compound formed from cations and anions held together by ionic bonds.

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Naming Ions

Metal ions use the same name as the atom, non-metal ions typically have ide added to the name.

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Ionic Compound Formula

Formulas for ionic compounds show the ratio of ions needed to achieve a neutral charge.

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Balancing Equations

Adjusting coefficients to ensure the same number of each atom type on both sides of the equation.

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pH Scale

A scale measuring acidity or alkalinity of a substance, ranging from 0 (most acidic) to 14 (least acidic). 7 is neutral.

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Acid

A substance that releases hydrogen ions (H+), is corrosive, tastes sour, and conducts electricity.

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Base

An alkaline substance that neutralizes acids, tastes bitter, and releases hydroxide ions (OH-).

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Neutralization Reaction

A reaction between an acid and a base that produces a salt and water.

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Acid-Carbonate Reaction

A reaction between an acid and a carbonate that produces a salt, water, carbon dioxide, and heat.

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Acid-Metal Reaction

A reaction between an acid and a metal that produces hydrogen gas and a salt.

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Half-Life

The time it takes for half of a radioactive substance to decay.

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Radioactive Decay

The process by which an unstable atomic nucleus loses energy by emitting radiation.

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Biotic Factor

A living or once-living component of an environment.

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Abiotic Factor

A non-living component of an environment.

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Asexual Reproduction

Reproduction without the fusion of gametes (sex cells).

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Binary Fission

Asexual reproduction where a single cell divides into two identical daughter cells.

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Budding

Asexual reproduction where a new organism grows from an outgrowth of the parent.

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Fragmentation

Asexual reproduction where a single organism breaks into pieces and each piece develops into a new organism.

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Parthenogenesis

Asexual reproduction in which an embryo develops from an unfertilized egg.

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Periodic Table Groups

Columns on the periodic table; elements in a group share similar chemical properties.

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Periodic Table Periods

Rows on the periodic table; elements in a period have increasing atomic number.

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Atomic Number

The number of protons in an atom's nucleus, uniquely identifying an element.

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Atomic Mass

The average mass of an atom, typically protons and neutrons.

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Metals (PT)

Elements on the left side of the periodic table, generally good conductors of electricity and heat.

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Nonmetals (PT)

Elements on the right side of the periodic table, generally poor conductors of electricity and heat.

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Metalloids (PT)

Elements with properties between metals and nonmetals, found in the middle of the periodic table.

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Alkali Metals

Highly reactive metals in Group 1 of the periodic table.

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Alkaline Earth Metals

Reactive metals in Group 2 of the periodic table.

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Halogens

Highly reactive nonmetals in Group 17 of the periodic table.

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Noble Gases

Unreactive nonmetals in Group 18 of the periodic table.

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Electrons

Negatively charged subatomic particles orbiting the nucleus.

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Protons

Positively charged subatomic particles in the nucleus.

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Neutrons

Neutral subatomic particles in the nucleus.

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Flame Tests

A laboratory technique used to identify metal ions by the color of the flame they produce.

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Sodium Chloride

Common table salt, a compound of sodium and chlorine.

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Carbon Dioxide

A colorless gas found in the atmosphere and produced by respiration.

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Nitrous Oxide

A colorless gas, used as a medicine and recreational drug.

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Valence Shell

The outermost electron shell of an atom.

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Atomic Stability

A state where an atom has a full valence electron shell and minimal energy.

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Reactivity

The tendency of an element to undergo a chemical change or reaction.

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Study Notes

Waves and Particle Model

  • Transverse Waves move perpendicular to the direction of the wave (e.g., water waves)
  • Longitudinal Waves move in the same direction as the energy (e.g., sound waves), including compressions and rarefactions.

Electromagnetic Spectrum

  • Radio Waves – communication
  • Microwaves – cooking
  • Infrared – heat transmission
  • Visible Light – (red, orange, yellow, green, blue, indigo, violet)
  • Ultraviolet – can cause cancer
  • X-rays – medical imaging
  • Gamma Rays – highly penetrating, kill cancer cells

Wavelength, Frequency & Speed

  • Wavelength—the distance from one trough to another.

Electricity and Energy

  • Electricity is measured in watts.
  • Energy is measured in joules.
  • Pitch is determined by frequency; higher frequency means higher pitch.

Law of Conservation of Energy

  • Energy cannot be created or destroyed; it can only be transformed or transferred.

Heat Energy

  • Heat moves from a hotter object to a cooler object until both are the same temperature.
  • Conduction: Heat transfer between objects in contact.
  • Convection: Heat transfer through fluids (liquids or gases).
  • Radiation: Heat transfer through space.

Sound and the Ear

  • Outer Ear: Pinna collects sound.
  • Middle Ear: Ear drum vibrates, ossicles transmit vibrations.
  • Inner Ear: Cochlea converts vibrations to electrical signals.
  • Process: Sound waves -> ear canal -> eardrum -> ossicles -> cochlea -> auditory nerve -> brain.

Light and the Eye

  • Lens: A curved transparent object that bends light.
  • Convex Lens: Fat in the middle, skinny on the sides.
  • Concave Lens: Skinny in the middle, fat on the sides.
  • Converging—moving towards one point.
  • Diverging—moving away from one point.

The Eye Structures

  • Cornea: Clear part of the sclera.
  • Iris: Controls pupil size.
  • Lens: Focuses light onto the retina.
  • Retina: Contains photoreceptors.
  • Optic nerve: Sends impulses to the brain.
  • Pupil: Hole in the eye that allows light to enter.
  • Sclera: Outside layer of the eye.

Reflection and Refraction

  • Reflect: Light bounces off a surface.
  • Diffuse Reflection: Light reflects at many different angles.
  • Refraction: Light bends as it passes through one medium to another.

The Five Senses

  • Touch, taste, smell, sight, hearing.

Senses and Control (Biology)

  • Receptors—sensory neurons—coordinators—motor neurons—effectors.
  • Stimuli—something that sets off a reaction.
  • Effectors—muscles/glands that respond to stimuli.
  • Reflex actions—quick responses to stimuli without brain involvement.

Nervous System and Neurons

  • Purpose: Detecting and responding to environmental changes.
  • Synapse: Connects neurons.
  • Neurons: Long cells carrying electrical signals.
  • Sensory Neurons: Collect external information.
  • Motor Neurons: Transmit messages to effectors.
  • Interneurons: Allow communication and perception.

Endocrine System

  • Purpose: Transmits messages via chemical signals (hormones).
  • Major Glands: Brain, thyroid, adrenal, pancreas, testes, ovaries

Homeostasis

  • Keeping the body balanced (temperature, blood levels, pH).
  • Negative Feedback Loop: Response to a change in a variable reverses that change.

Male Reproductive System

  • Testes - Sperm production.
  • Scrotum: Maintains temperature for sperm.
  • Epididymis; Tubes that carry sperm to the vas deferens.
  • Seminal Vesicles; Adds fluids to the sperm and semen.

Female Reproductive System

  • Ovaries - Egg release.
  • Fallopian tubes - transport eggs.
  • Uterus - Development of the embryo.
  • Vagina - Birth canal.

Fertilisation and Pregnancy

  • When sperm and egg fuse, forming a zygote.

Labour & Birth

  • Dilation
  • Expulsion
  • Delivery of placenta

Immune System - Line of Defence

  • First line: Barriers (skin, mucus membranes).
  • Second line: Non-specific responses (inflammation, fever).
  • Third line: Targeted immune response (antibodies, lymphocytes).

Nutrition & Disease

  • Nutritional diseases: Caused by nutrient deficiencies.
  • Infectious diseases: Caused by pathogens.
  • Vaccination: Exposure to a less harmful form of pathogen to build immunity.

Asexual and Sexual Reproduction

  • Asexual reproduction: Create genetic copies of oneself without another organism.
  • Sexual reproduction: Combination of genetic material from two parents.

Periodic Table

  • Groups—columns.
  • Periods—rows.
  • Atomic Number—number of protons.
  • Atomic Mass—weight of protons and neutrons.
  • Elements grouped by properties.
  • Metalloids; Properties between metals and non metals.

Atom Structure

  • Electrons orbit the nucleus.
  • Protons are positively charged.
  • Neutrons have no charge.

Flame Tests

  • Identifying metal ions by the color the flame emits.

Reactivity & Stability

  • Atom stability—full valence shell.
  • Reactivity depends on valence electrons and distance from the nucleus.

Ionic Bonding

  • Atoms gaining or losing electrons to form ions (cations and anions).

Compounds & Formulae

  • Combining elements in specific ratios.
  • Balancing chemical equations, making sure the same number of atoms of each kind appear on both sides of the equation.

Electron Diagrams

  • Visual representation of electrons in atoms.
  • Lewis dot diagrams—show valence electrons.

Acid-Base Reactions

  • pH scale (0-14), neutral pH is 7.
  • Acids have hydrogen ions (H+); Bases have hydroxide ions (OH-).
  • Neutralization: Acids and bases react to form a salt and water.

Radioactivity

  • Half-life: Time for half of a radioactive material to decay.
  • Types of radiation: Alpha, beta, gamma.
  • Uses of radioactivity: Medicine, research.

Biotic and Abiotic Factors

  • Biotic: Living things in an environment.
  • Abiotic: Non-living components of an environment.

Ecosystem

  • Interactions between biotic and abiotic factors.

Food Chains, Food Webs, and Energy Flows

  • Producers, consumers, and decomposers.

The Cycles (e.g., Carbon, Nitrogen, Phosphorus)

  • Biogeochemical cycles—the cycling of elements through the Earth.
  • Details of each cycle.

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