4.1 Notes
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The document discusses the history and development of atomic models from ancient Greek philosophers to modern scientific theories. It describes Democritus' idea that atoms are the smallest indivisible particles of matter. John Dalton proposed his atomic theory that all matter is composed of atoms of different elements that combine in fixed ratios. J.J. Thomson's experiments provided evidence that atoms contain smaller charged particles, leading to his "chocolate chip" atomic model. Finally, Rutherford discovered the atomic nucleus by observing alpha particle scattering, realizing that the positive charge and mass of atoms are concentrated in a tiny nucleus.
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History of atoms
Greek philosopher Democritus first proposed the idea of atoms in 460 BC, reasoning that matter must be divisible into indivisible particles. However, his idea was largely ignored. In the early 1800s, John Dalton performed experiments and developed an atomic theory, stating that elements are made of identical atoms that combine to form compounds. In 1897, Joseph John Thomson discovered the electron and proposed a early atomic model where electrons were embedded in a uniform sphere of positive charge, like raisins in pudding, known as the plum pudding model.
Development of Atomic Theory
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
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HISTORY OF ATOMIC THEORY
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
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- J.J. Thomson's plum pudding model of the atom was modified based on evidence from experiments by Rutherford, Geiger, Marsden, and Bohr.
- In the gold foil experiment, Geiger and Marsden observed some alpha particles deflected at high angles from a thin gold foil, inconsistent with Thomson's model but evidence for a small, dense nucleus.
- Bohr incorporated Planck's quantum theory to explain the stability of atoms, suggesting electrons occupy discrete energy levels and jump between them.
History of atomic theory
Early philosophers proposed that all matter was made of tiny indivisible particles called atoms. John Dalton later proposed the first atomic theory with evidence, stating that atoms are uniform spheres that make up elements. J.J. Thomson's experiments discovered the electron, showing atoms contain negatively charged particles. Rutherford's experiments demonstrated that atoms have small, dense positively charged nuclei surrounded by empty space occupied by electrons. This led to the modern understanding of atomic structure with protons, neutrons, and electrons.
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The document outlines the major theories in the development of atomic theory from ancient Greece to the 20th century. It describes the key contributors including:
Democritus who proposed that all matter is made of basic elements composed of indivisible atoms. John Dalton introduced the modern concept of atoms as basic units of elements that combine in fixed ratios. J.J. Thompson discovered the electron and proposed the plum pudding model where electrons are distributed in a positive charge. Ernest Rutherford discovered the nucleus through alpha particle experiments and proposed atoms have a small, dense positively charged nucleus. Niels Bohr incorporated quantum theory and proposed electrons orbit in fixed shells around the nucleus. Finally, Schrodinger and Heisenberg developed the quantum
Atomic structure history_dem_to_bohr
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
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History of atoms
Greek philosopher Democritus first proposed the idea of atoms in 460 BC, reasoning that matter must be divisible into indivisible particles. However, his idea was largely ignored. In the early 1800s, John Dalton performed experiments and developed an atomic theory, stating that elements are made of identical atoms that combine to form compounds. In 1897, Joseph John Thomson discovered the electron and proposed a early atomic model where electrons were embedded in a uniform sphere of positive charge, like raisins in pudding, known as the plum pudding model.
Development of Atomic Theory
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
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The history of the atomic theories from Democritus until Bohr's atomic theories. (IB Chemistry HL - Chapter 2: Atomic Structures)
HISTORY OF ATOMIC THEORY
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
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- J.J. Thomson's plum pudding model of the atom was modified based on evidence from experiments by Rutherford, Geiger, Marsden, and Bohr.
- In the gold foil experiment, Geiger and Marsden observed some alpha particles deflected at high angles from a thin gold foil, inconsistent with Thomson's model but evidence for a small, dense nucleus.
- Bohr incorporated Planck's quantum theory to explain the stability of atoms, suggesting electrons occupy discrete energy levels and jump between them.
History of atomic theory
Early philosophers proposed that all matter was made of tiny indivisible particles called atoms. John Dalton later proposed the first atomic theory with evidence, stating that atoms are uniform spheres that make up elements. J.J. Thomson's experiments discovered the electron, showing atoms contain negatively charged particles. Rutherford's experiments demonstrated that atoms have small, dense positively charged nuclei surrounded by empty space occupied by electrons. This led to the modern understanding of atomic structure with protons, neutrons, and electrons.
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The document outlines the major theories in the development of atomic theory from ancient Greece to the 20th century. It describes the key contributors including:
Democritus who proposed that all matter is made of basic elements composed of indivisible atoms. John Dalton introduced the modern concept of atoms as basic units of elements that combine in fixed ratios. J.J. Thompson discovered the electron and proposed the plum pudding model where electrons are distributed in a positive charge. Ernest Rutherford discovered the nucleus through alpha particle experiments and proposed atoms have a small, dense positively charged nucleus. Niels Bohr incorporated quantum theory and proposed electrons orbit in fixed shells around the nucleus. Finally, Schrodinger and Heisenberg developed the quantum
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1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
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1. J.J. Thomson discovered electrons in cathode ray tubes and concluded they were negatively charged particles smaller than atoms.
2. In the gold foil experiment, Rutherford expected alpha particles to pass through or be slightly deflected, but some were deflected at large angles or rebounded, indicating the positive charge was concentrated in a small nucleus.
3. This led Rutherford to propose the nuclear model of the atom with electrons orbiting a small, dense positively charged nucleus.
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1) Early Greek philosopher Democritus proposed that all matter is made of tiny, indivisible particles called atoms.
2) In the early 1800s, English scientist John Dalton developed the first serious atomic theory, proposing that elements are made of atoms and atoms of the same element have the same properties.
3) J.J. Thomson's discovery of the electron in 1897 showed that atoms contain smaller subatomic particles, challenging the idea that atoms are indivisible.
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Democritus was one of the first to propose the idea of atoms in 440 BCE, suggesting that matter is made up of tiny indivisible particles called atoms. In the early 1900s, experiments led scientists to develop more accurate models of the atom. Rutherford discovered the nucleus in 1909 by firing positively charged particles at a gold foil and observing some particles deflecting, indicating a small, dense nucleus. Bohr then proposed in 1913 that electrons orbit the nucleus in distinct energy levels. The modern atomic theory describes the regions where electrons are likely to be found as electron clouds.
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Dalton's atomic theory proposed that matter is made of small indivisible particles called atoms, atoms of the same element are identical, and atoms of different elements have different masses and properties. Rutherford discovered the nucleus of the atom through his gold foil experiment, finding that some alpha particles bounced off the small, dense nucleus at the center of the atom. Chadwick discovered the neutron through experiments with excessively charged atoms, an uncharged particle that helped explain nuclear structure.
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1) The Democritus model from 400 BC proposed that all matter is made of invisible indivisible particles called atoms.
2) J.J. Thomson's "plum pudding" model from the 1900s depicted atoms as uniform spheres of positive matter containing embedded electrons.
3) Rutherford's gold foil experiments in 1911 led him to propose a planetary model with electrons orbiting a small, positively charged nucleus.
4) Niels Bohr's 1913 model explained atomic spectra by proposing electrons orbit in fixed energy levels around the nucleus.
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- Theories of atomic structure have evolved over time from early Greek philosophers' ideas of basic elements to J.J. Thomson's discovery of electrons and Rutherford's discovery of the dense atomic nucleus at the center, surrounded by orbiting electrons.
- Modern atomic theory incorporates concepts like Bohr's planetary model of electron orbits and specific energy levels within atoms.
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2. In the gold foil experiment, Rutherford expected alpha particles to pass through or be slightly deflected, but some were deflected at large angles or rebounded, indicating the positive charge was concentrated in a small nucleus.
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1) Early Greek philosopher Democritus proposed that all matter is made of tiny, indivisible particles called atoms.
2) In the early 1800s, English scientist John Dalton developed the first serious atomic theory, proposing that elements are made of atoms and atoms of the same element have the same properties.
3) J.J. Thomson's discovery of the electron in 1897 showed that atoms contain smaller subatomic particles, challenging the idea that atoms are indivisible.
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Democritus was one of the first to propose the idea of atoms in 440 BCE, suggesting that matter is made up of tiny indivisible particles called atoms. In the early 1900s, experiments led scientists to develop more accurate models of the atom. Rutherford discovered the nucleus in 1909 by firing positively charged particles at a gold foil and observing some particles deflecting, indicating a small, dense nucleus. Bohr then proposed in 1913 that electrons orbit the nucleus in distinct energy levels. The modern atomic theory describes the regions where electrons are likely to be found as electron clouds.
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Dalton's atomic theory proposed that matter is made of small indivisible particles called atoms, atoms of the same element are identical, and atoms of different elements have different masses and properties. Rutherford discovered the nucleus of the atom through his gold foil experiment, finding that some alpha particles bounced off the small, dense nucleus at the center of the atom. Chadwick discovered the neutron through experiments with excessively charged atoms, an uncharged particle that helped explain nuclear structure.
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The atomic theory has evolved over time based on new discoveries. Early philosophers proposed that all matter is made of indivisible particles called atoms. In the early 1800s, scientists proposed that atoms of different elements have distinct properties and combine in fixed ratios. At the turn of the 20th century, experiments revealed internal structures of atoms including electrons, protons, and nuclei. Later work determined the composition and arrangement of these subatomic particles, leading to modern atomic theory that atoms are made of protons, neutrons, and electrons with electrons orbiting the nucleus.
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The document summarizes the major historical models of atomic structure:
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2) J.J. Thomson's "plum pudding" model from the 1900s depicted atoms as uniform spheres of positive matter containing embedded electrons.
3) Rutherford's gold foil experiments in 1911 led him to propose a planetary model with electrons orbiting a small, positively charged nucleus.
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This document discusses early atomic theories and models of matter. It describes the theories of Aristotle, who believed that matter was continuous with no empty spaces, and Democritus, who proposed that matter was discontinuous and could be divided into smaller particles called atoms. The document then focuses on John Dalton's atomic model from the early 1800s, which proposed that all matter is composed of atoms, atoms of the same element are identical, atoms of different elements differ, and atoms combine in chemical reactions. Dalton's model helped establish the foundations of modern atomic theory.
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The document traces the development of atomic models from ancient Greek philosophers who proposed atoms as fundamental units of matter, to modern scientific understanding. Key developments include Dalton's atomic theory which established atoms as indivisible particles that combine in simple whole number ratios, and Rutherford's nuclear model which placed a dense positively charged nucleus at the atom's center surrounded by orbiting electrons. Later models incorporated the discoveries of subatomic particles like protons, neutrons, and electrons that make up atoms and occupy certain energy levels or orbitals. While historic models were limited by available evidence, each contributed important concepts that advanced the understanding of atomic structure over time.
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The document summarizes the history and development of atomic theory from ancient Greek philosophers to modern quantum mechanics. It describes early theories proposed by Aristotle and Democritus. John Dalton rejected Aristotle's theory and proposed atoms are indivisible, identical for each element, and combine in whole number ratios. Discovery of the electron, proton, and neutron led to new atomic models. Quantum mechanics explains atomic structure as electrons occupying probabilistic orbitals rather than fixed paths. The current model integrates discoveries of subatomic particles and quantum theory.
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- Modern atomic theory incorporates concepts like Bohr's planetary model of electron orbits and specific energy levels within atoms.
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The document describes how scientific theories of the atom have changed over time. Early Greek philosophers like Democritus proposed that matter was made of indivisible particles called atoms, though there was no evidence. In the 1800s, John Dalton proposed the billiard ball model where all atoms of an element were identical. J.J. Thomson later discovered the "plum pudding" model with electrons in a positive sphere. Ernest Rutherford then found atoms have a dense positive nucleus with electrons in orbits around it. Niels Bohr added that electrons exist in certain energy levels. Later, Schrodinger and Heisenberg developed the electron cloud model where electrons' positions are uncertain within orbital regions.
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1) Atoms are composed of a small, dense, positively charged nucleus surrounded by negatively charged electrons.
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3) Atoms of the same element have the same number of protons but can vary in the number of neutrons, resulting in different isotopes of that element with different atomic masses.
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Atom History PP.ppt
1. Atomic theory has evolved over time from early Greek philosophers' idea of invisible atoms to modern quantum mechanical models.
2. Rutherford's gold foil experiment in the early 1900s revealed that atoms have a small, dense nucleus surrounded by empty space, overturning the plum pudding model.
3. Niels Bohr incorporated Rutherford's findings into his 1913 model where electrons orbit the nucleus in distinct energy levels, though later quantum mechanics describes electron location as a probability cloud rather than distinct orbits.
Atomic Structure
The document discusses the history and development of atomic theory from ancient Greek philosophers to modern scientists like Dalton, Thomson, Rutherford, and Bohr. It explains key concepts like atoms being the smallest particle of an element that retains its properties, atomic number representing the number of protons, isotopes being variants of the same element with different numbers of neutrons, and the discovery of subatomic particles like protons, neutrons, and electrons that make up the tiny nuclear structure of atoms.
Minooka - Elements Part 2
Atoms are the smallest particles of elements that retain their chemical properties. Atoms consist of protons, neutrons, and electrons. John Dalton proposed his atomic theory in 1808, stating that all matter is made of indivisible atoms, atoms of the same element are identical, and atoms combine in simple whole number ratios. In the early 1900s, experiments showed that atoms have a small, dense nucleus surrounded by electrons, and electrons can exist in certain energy levels or orbits around the nucleus.
Atomic Theory Overview
The document summarizes the historical development of atomic structure models from ancient philosophers to modern atomic theory. It describes early continuous models proposed by Aristotle and Democritus' earliest concept of atoms. John Dalton established the foundations of modern atomic theory by proposing atoms as indivisible particles that combine in whole number ratios. J.J. Thomson's experiments led him to propose a "plum pudding" model with electrons embedded in a positive sphere. Rutherford determined atoms have a small, dense positively charged nucleus surrounded by electrons. Modern atomic structure incorporates discoveries by Bohr and Chadwick that atoms consist of a nucleus of protons and neutrons surrounded by electrons in shells.
Atomic Theory Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental indivisible units of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing positive charge.
3. Later models like Bohr's incorporated the idea that electrons orbit the nucleus in fixed energy levels, accounting for the emission and absorption of photons.
A T O M I C T H E O R Y Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental building blocks of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing most of its mass.
3. Later discoveries found that the nucleus contains protons and neutrons, while electrons orbit the nucleus, leading to the modern understanding of atomic structure.
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24 1 the atmosphere
The atmosphere is composed primarily of nitrogen, oxygen, and other gases that surround the Earth. It protects the Earth from harmful rays from the sun while trapping heat, and provides conditions suitable for life. The atmosphere consists of four main layers - the troposphere, stratosphere, mesosphere, and thermosphere - with decreasing air pressure and density at higher altitudes. The stratosphere contains the ozone layer which absorbs UV rays.
Ch 18 5 sources of light
There are several sources of light described in the document. Incandescent light bulbs produce light as electrons flow through a heated filament. Fluorescent lights emit light by causing a phosphor to emit photons through a series of collisions that change wavelengths into visible light. Laser light is a beam of coherent light emitted when excited atoms release photons; it maintains a constant intensity. Sodium-vapor lights ionize gas mixtures in a bulb, causing sodium to emit light as electrons move between energy levels upon heating.
Ch 18 4 colors
White light separates into colors when passing through a prism due to different wavelengths refracting at different angles, called dispersion. An object's color depends on both its composition and the color of light illuminating it. Primary colors are red, green, and blue, which when mixed in different amounts can create all other colors. Secondary colors are cyan, yellow, and magenta, which are combinations of two primary colors. Complimentary colors of light combine to form white light. Primary pigment colors are cyan, yellow, and magenta.
Ch 18 2 electromagnetic spectrum
The electromagnetic spectrum includes various types of waves ranging from radio waves to gamma rays. Radio waves are used for radio, television, radar, and microwaves, which can be used to cook food. The electromagnetic spectrum also includes infrared rays, visible light, ultraviolet rays, X-rays, and gamma rays, each with their own characteristics and applications such as medicine, agriculture, imaging internal structures, and cancer treatment.
Ch 18 1 electromagnetic waves
Electromagnetic waves consist of changing electric and magnetic fields that can travel through matter or empty space, transferring energy. They are produced when electric charges vibrate or accelerate and all travel at the same speed in a vacuum, as measured by Michelson. While wavelength and frequency vary inversely, electromagnetic radiation behaves both as waves and particles, with intensity decreasing with distance from the source as photons disperse.
15.1 notes
The document discusses different forms of energy including kinetic energy, which depends on an object's mass and speed, and potential energy, which can be gravitational or elastic. It provides examples of calculating kinetic energy for a flying bird and gravitational potential energy for a diver. The document also categorizes the main forms of energy as mechanical, thermal, chemical, electrical, electromagnetic, and nuclear, and notes that nuclear power plants use nuclear energy to generate electricity by splitting atoms to heat water and spin turbines.
11 3 acceleration section
Acceleration is defined as a change in an object's speed or direction over a period of time. It can be calculated by taking the change in velocity (final velocity minus initial velocity) divided by the time taken. Acceleration is measured in meters per second squared. Slowing down is considered deceleration or negative acceleration. Constant acceleration results in a steady change in velocity at the same rate over time and is represented by a straight line on a graph where the slope equals the acceleration.
3.1 notes
The document discusses the differences between solids, liquids, and gases. Solids have a definite shape and volume, do not compress, and do not assume the shape of their container. Liquids have no definite shape but a definite volume, cannot be compressed, and assume the shape of their container. Gases have no definite shape or volume, can be compressed, and assume the shape of their container. The kinetic theory states that particles in all matter are in constant motion and the behavior of gases is due to the fast, random motion of particles which overcome attractive forces between them.
2.2 notes
Physical properties are characteristics that can be observed or measured without changing a substance's composition, and include viscosity, conductivity, malleability, hardness, melting point, boiling point, and density. These properties can be used to identify materials, determine which are best for specific uses, and separate mixtures through processes like filtration and distillation.
2.1 notes
This document classifies matter as either pure substances or mixtures. Pure substances are uniform throughout and can be elements, which contain only one type of atom, or compounds, which contain two or more elements joined together. Mixtures are not uniform and can be either heterogeneous, with noticeably different parts, or homogeneous, with evenly distributed parts. Mixtures are further classified as solutions, suspensions, or colloids based on the size of particles in the mixture.
2.2 notes
Physical properties are characteristics that can be observed or measured without changing the composition of a substance. Some key physical properties include viscosity, conductivity, malleability, hardness, melting point, boiling point, and density. Physical properties can be used to identify materials, determine which are best suited for specific uses, and separate mixtures using techniques like filtration and distillation.
1.2 notes
The document outlines the scientific method which involves making observations, conducting research to form a hypothesis, testing the hypothesis through controlled experiments and data collection, drawing a conclusion, and potentially developing a new theory. It also discusses key aspects of the scientific method including forming testable hypotheses with manipulated and responding variables, controlling outside factors, revising hypotheses not supported by evidence, and how scientific laws summarize patterns in nature while theories aim to explain them. Scientific models are also mentioned as tools to visualize complex concepts.
How to make a good graph
To make a good graph, include a title, labels for the axes, and consistent scales. The x-axis should include the independent variable like time, while the y-axis includes the dependent variable measured. Data points can be connected with a smooth curve to show patterns, and less ink allows easier readability. Key details like calculations or uncertainties should be indicated on the graph as needed.
1.4 notes
Scientists use various visual formats like tables, line graphs, bar graphs, and circle graphs to organize and present data. Tables relate variables and display values in rows and columns. Line graphs show changes over time or between variables with slope indicating relationships. Bar graphs compare measurements, while circle graphs illustrate proportions of a whole.
1.3 notes
Scientific notation and SI units are used in measurement to help scientists communicate measurements clearly across countries. The basic SI units include meters, kilograms, seconds, amperes, moles, candelas, and kelvins. Derived units are calculated from the basic units, such as newtons from kilograms and meters/seconds. SI prefixes modify the scale of units, from centi to giga. The precision of calculations is limited by the measurement with the fewest significant figures. Temperature in kelvins is calculated by adding 273 to degrees Celsius.
1.2 notes
The document outlines the scientific method which involves making observations, conducting research to form a hypothesis, testing the hypothesis through controlled experiments and data collection, drawing a conclusion, and potentially developing a new theory. It also discusses key aspects of the scientific method including forming testable hypotheses with manipulated and responding variables, controlling outside factors, revising hypotheses not supported by evidence, and how scientific laws summarize patterns in nature while theories aim to explain them and cannot be proven. Scientific models are also mentioned as helping visualize complex concepts.
Ch 1 1 notes
Science begins with curiosity and uses methods to discover knowledge. It includes natural sciences like physical science, chemistry, physics, earth and space science, as well as life sciences concerning living things. Physical science covers big ideas like space and time, matter and change, forces and motion, and energy.
Ch 26-1 The sun
The document summarizes key aspects of energy from the sun and its atmospheric features. The sun's energy comes from nuclear fusion reactions in its core that convert hydrogen into helium. This outward pressure is balanced by the sun's inward gravitational force, maintaining stability. The sun's atmosphere has three layers - the visible photosphere, the middle chromosphere, and the outer corona containing hot gases that flow out as solar winds. Sunspots, prominences, and solar flares are prominent atmospheric features.
Groups of stars 26.4
Star systems consist of two or more stars held together by gravity, with over half of all stars existing in systems. Star clusters form when stars are born together in the same nebula, allowing their ages to be determined. The three types of star clusters are open clusters, associations, and globular clusters. Galaxies are classified into four main categories: spiral, barred-spiral, elliptical, and irregular galaxies, which can be distinguished by their shapes, presence of spiral arms, and stages of star formation.
Evolution of a star 26 3
Stars form from dense regions in nebulae where dust and gases heat up and contract to form a protostar with enough mass for nuclear fusion to begin. Most stars will spend around 90% of their life as a main sequence star stably fusing hydrogen into helium. A star's mass determines its place on the main sequence, with smaller, cooler red stars living the longest. Lower mass stars eventually become white dwarfs as their cores grow without outward pressure, while higher mass stars explode as supernovae, leaving behind neutron stars or black holes if the core is massive enough for its surface gravity to trap even light.
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