Notes lab 04 ions and isotopes
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Atoms of the same element can exist with different numbers of neutrons, called isotopes. Isotopes are written with the element symbol and mass number, such as C14 for the carbon isotope with 6 protons and 8 neutrons. Ions are atoms that have gained or lost electrons, giving them a positive or negative charge and making them no longer neutral. Atoms gain electrons to become negative ions and lose electrons to become positive ions.
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Notes lab 04c ions and isotopes
Atoms of the same element can exist with different numbers of neutrons, called isotopes, which are identified by elemental symbol and mass number. Ions are atoms that have gained or lost electrons, giving them a positive or negative electrical charge and making them positive or negative ions, respectively. Atoms are normally electrically neutral unless bonding occurs.
Unit 1 lesson 12ppt
When a neutral atom loses or gains electrons, it is no longer neutral. It becomes an ion that has a positive or negative charge depending on whether electrons were lost or gained:
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing or gaining electrons changes a neutral atom's charge balance between protons and electrons, making it an ion that is positively or negatively charged. The number of protons does not change, only the number of electrons.
Unit 1 lesson 12ppt
When a neutral atom loses or gains electrons, it is no longer electrically balanced. It will have either a positive or negative charge depending on whether it lost or gained electrons.
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing electrons creates a positive ion and gaining electrons creates a negative ion. The charge depends on the relative numbers of protons and electrons after gaining or losing electrons from the neutral atom.
How many electrons?
The document discusses isotopes, ions, atomic numbers, and atomic masses. It defines isotopes as atoms of the same element that have varying numbers of neutrons. It notes that ions are atoms with unequal numbers of protons and electrons, making them positively or negatively charged. For neutral atoms, the number of protons equals the number of electrons and is equal to the atomic number. The document also provides examples of calculating the number of protons, neutrons, and electrons for different atoms and ions.
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2) The nucleus contains an equal number of protons and electrons, giving the atom a neutral charge.
3) An example is provided for aluminum, showing its atomic number, number of protons and electrons.
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2. When the switch is closed, current flows in the circuit and the lights turn on.
3. There are two main types of voltage sources: direct current (DC) sources like batteries; and alternating current (AC) sources like generators.
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The document discusses atomic structure and isotopes. It recaps atomic structure, including the structure of the atom, relative masses and charges of protons, neutrons and electrons, chemical symbols, and electronic configuration. It then defines isotopes as atoms of the same element that contain the same number of protons but different numbers of neutrons. Examples of isotopes of oxygen are provided. Finally, some uses of radioactive isotopes are mentioned, such as in food irradiation, archaeological dating, smoke detectors, and as radioactive tracers.
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The document discusses how atoms form bonds. It states that atoms form bonds using electrons in their outer energy levels, and that there are four ways atoms can bond: by losing electrons, gaining electrons, pooling electrons, or sharing electrons. It then focuses on the specific ways that sodium and chlorine atoms form bonds by gaining and losing electrons. Sodium loses an electron to achieve a stable electron configuration, becoming a positively charged sodium ion (Na+). Chlorine gains an electron to achieve stability, becoming a negatively charged chloride ion (Cl-). These oppositely charged ions are then attracted to each other, forming an ionic bond and the compound sodium chloride (table salt). The document also notes that elements can lose or gain
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Notes lab 04c ions and isotopes
Atoms of the same element can exist with different numbers of neutrons, called isotopes, which are identified by elemental symbol and mass number. Ions are atoms that have gained or lost electrons, giving them a positive or negative electrical charge and making them positive or negative ions, respectively. Atoms are normally electrically neutral unless bonding occurs.
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When a neutral atom loses or gains electrons, it is no longer neutral. It becomes an ion that has a positive or negative charge depending on whether electrons were lost or gained:
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing or gaining electrons changes a neutral atom's charge balance between protons and electrons, making it an ion that is positively or negatively charged. The number of protons does not change, only the number of electrons.
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When a neutral atom loses or gains electrons, it is no longer electrically balanced. It will have either a positive or negative charge depending on whether it lost or gained electrons.
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing electrons creates a positive ion and gaining electrons creates a negative ion. The charge depends on the relative numbers of protons and electrons after gaining or losing electrons from the neutral atom.
How many electrons?
The document discusses isotopes, ions, atomic numbers, and atomic masses. It defines isotopes as atoms of the same element that have varying numbers of neutrons. It notes that ions are atoms with unequal numbers of protons and electrons, making them positively or negatively charged. For neutral atoms, the number of protons equals the number of electrons and is equal to the atomic number. The document also provides examples of calculating the number of protons, neutrons, and electrons for different atoms and ions.
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This document provides information about atomic structure:
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1. Electromotive force (emf) is the potential difference between the poles of a battery when it is not draining current in an open circuit.
2. When the switch is closed, current flows in the circuit and the lights turn on.
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Here are the key steps to solve this problem:
1) Isotope 35Cl has a relative abundance of 75.8%
2) Isotope 37Cl has a relative abundance of 24.2%
3) The relative atomic mass of 35Cl is 35 amu
4) The relative atomic mass of 37Cl is 37 amu
5) Use the formula: Relative Atomic Mass = Σ (Relative Abundance of isotope x Atomic Mass of isotope)
6) For 35Cl: Relative Abundance = 75.8%, Atomic Mass = 35 amu. So, contribution is 75.8% of 35 = 26.43
7) For 37Cl: Relative Abundance = 24
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3) Electrons fill the lowest available shell around the nucleus. The arrangement of electrons is shown in an element's electronic structure.
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Here are the key steps to solve this problem:
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This document discusses key objectives and terms related to the behavior of light waves and their interaction with mirrors and lenses. The objectives are to investigate light wave interactions, predict image characteristics formed by lenses and mirrors, and describe light wave behavior including reflection, refraction, diffraction and interference. Key terms defined include law of reflection, reflection, plane mirror, concave mirror, convex mirror, refraction, concave lens, convex lens. Characteristics of images formed by different mirror and lens types are also outlined.
Notes pb lab 06 part 1 the spactacular spectrum
The document discusses the electromagnetic spectrum and key objectives for students to understand it. It explains that the electromagnetic spectrum includes seven types of electromagnetic waves - radio waves, microwaves, infrared waves, visible light, ultraviolet light, X-rays, and gamma rays - which are arranged based on their wavelength and frequency. The document provides information about each type of electromagnetic wave, their properties, typical uses, and proportion of the overall spectrum. The objectives are for students to investigate and understand electromagnetic waves, compare the different types, describe applications of each type, and recognize that electromagnetic waves can travel without a medium.
Notes pb lab 06 part 2 the spectacular spectrum separating light
The document discusses spectranomy and how prisms can be used to separate light into a continuous spectrum. It provides examples of bright line spectra for various elements like mercury, hydrogen, nitrogen, argon, and neon that can be used to identify unknown elements. The end discusses the stars Rigel and Betelgeuse in the constellation Orion.
Notes pb lab 08 sounds cool
The document discusses key concepts about sound waves, including resonance, interference, and their everyday examples. Resonance occurs when sound waves travel in phase, causing another object to vibrate at the same frequency. Interference is the combination of two or more waves resulting in a change in sound quality - if it improves the quality, it is constructive interference; if it lessens the quality, it is destructive interference. The document also lists several essential learnings about the nature and properties of sound waves.
Notes pb lab 05 making waves
The document discusses two types of waves: transverse waves and longitudinal waves. Transverse waves have energy that moves perpendicular to the direction of the wave. Examples include light and water waves. Longitudinal waves have energy that moves parallel to the direction of the wave and require a medium, like sound waves. Key characteristics of both waves include wavelength, frequency, and amplitude. The document also provides diagrams and videos to illustrate these two wave types.
Notes pb lab 05 making waves lab check
This document discusses transverse and longitudinal waves. It defines key terms like amplitude, crest, and trough for transverse waves and compression and rarefaction for longitudinal waves. It notes that transverse waves can travel through empty space while longitudinal waves require a medium. Videos are linked to demonstrate both wave types and their differences in how energy travels - perpendicular for transverse waves and parallel for longitudinal waves. Characteristics of each wave type are summarized.
Notes pb lab 04 go with the flow
This document provides information about electrical circuits. It defines key terms like current, resistance, resistors, series circuits and parallel circuits. It explains that series circuits provide only one path for electrons to flow while parallel circuits provide multiple paths. The document notes that resistance affects current differently in each circuit type and that current increases directly with voltage but inversely with resistance. It emphasizes that understanding these relationships is an essential learning.
Notes pb lab 03c the big switch motor only
This document asks several questions about how motors work and what materials and energy are needed to make a basic motor. It asks what kind of energy is required to power a motor, why wire is coiled around the center axle, and why there are two different colored magnets inside the steel can of the motor. It also asks what materials and energy source would be needed to make a simple motor.
Notes pb lab 03b the big switch
This document discusses electromagnetic induction and how motors and generators work. It defines key terms like electromagnet, electric field, magnetic field, induction. It explains that a motor converts electrical energy to mechanical energy using electromagnetic induction to create opposing electromagnetic fields on an armature that spin it. A generator converts mechanical energy to electrical energy by passing a coil through a magnetic field, inducing current. Both have coils and magnets but differ in the direction of energy flow and transformation. The document is titled "The Big Switch" because the same device can function as a motor or generator depending on the direction of energy and force.
Notes pb lab 03a the big switch introduction
This document discusses static electricity and how electricity is generated and used. It asks questions about how electricity is produced, whether static electricity from moving legs could power a headlight, how generators use magnets to generate electricity, why iron filings arrange around magnets, what energy is needed to power a motor and where it comes from, why wire is coiled around the center of an axle, why magnets inside a steel can have different colors, what materials and energy would be needed to make a motor, and how a flashlight works.
Notes pb lab 02 wheres the juice
This document provides information about key terms related to batteries, including electrodes, electrolytes, voltage, and potential difference. It explains that electrodes are the metal or carbon elements that react with an electrolyte, usually a liquid acid or base, to produce voltage. A wet cell battery requires a strong acid or base electrolyte, while a dry cell uses a dry paste electrolyte. The document is intended to help students better understand how electricity is created in wet and dry cell batteries through vocabulary terms and by identifying the necessary parts of each type of battery.
Notes pb lab 01c energy transformations 2 vocabulary notes
This document discusses different types of energy including thermal, chemical, electrical, radiant, nuclear, and mechanical energy. It provides examples for each type of energy. Thermal energy is the energy of moving molecules, chemical energy comes from atomic rearrangement during chemical reactions like in batteries, and electrical energy comes from electron flow measured in volts and amperes. Radiant energy travels in waves from a source like the sun. Nuclear energy comes from atomic nuclei combining or splitting. Mechanical energy can be kinetic from motion or potential from stored energy like a ball at the top of a ramp. The document also discusses energy chains, sources, receivers, and the law of conservation of energy. Nuclear energy occurs through fission which splits atoms or
Notes gb lab 11 disappearing powde investigating solubility
The document defines key terms related to solubility including solvent, solute, solution, mixture, and saturation point. It explains that solubility is a characteristic property expressing the maximum amount of solute that will dissolve in a solvent. The document also notes that the point where the x and y axes intersect on a solubility graph is called the saturation point. It provides tips for increasing the rate at which a solute dissolves, such as increasing surface area, temperature, or rate of mixing.
Notes gb lab 10 names bond ionic bond 02
The document summarizes the key characteristics of ionic and covalent bonds. It states that ionic bonds form between metals and nonmetals through the transfer of valence electrons from the metal to the nonmetal. Covalent bonds form between nonmetals and between like atoms through the sharing of valence electrons. The document also notes that conductivity testing can be used to distinguish between ionic compounds with high conductivity and covalent compounds with low conductivity.
Notes gb lab 10 names bond ionic bond 01
The document discusses the characteristics of ionic and covalent bonds. It explains that ionic bonds form between metals and nonmetals through the transfer of valence electrons from the metal to the nonmetal. Covalent bonds form between nonmetals and involve the sharing of valence electrons between atoms. The type of bond can be identified by measuring the conductivity of compounds, with ionic compounds being highly conductive and covalent compounds being poorly conductive.
Notes gb lab 09 colorful chemicalp h scale
Acids and bases are chemical compounds that are defined by their properties in aqueous solutions and chemical reactions. Acids are compounds that donate hydrogen ions (H+) in water, turning litmus paper red and reacting with bases. Bases are compounds that accept hydrogen ions in water, turning litmus paper blue and neutralizing acids in a reaction that produces water.
Notes gb lab 09 colorful chemical clues 1
The document provides information about acids and bases for students. It defines acids as compounds that produce hydrogen ions in water and have a sour taste and corrode metals. Bases are defined as compounds that produce hydroxide ions in water and have a bitter taste. It introduces pH as a measure of acidity on a scale from 1-14, with 1 being the strongest acid and 14 the strongest base. Indicators are described as tools that change color to identify acids and bases. Key concepts covered include neutralization reactions, reactivity, and examples of common acids and bases.
Notes gb lab 08 endothermic and exothermic reactions
The document discusses endothermic and exothermic chemical reactions. It defines endothermic reactions as those that require continuous energy input and cause temperature to decrease, while exothermic reactions release energy and cause temperature to increase. Examples of each type of reaction are given, like endothermic barium hydroxide mixing and exothermic glow sticks. Line graphs are used to illustrate temperature changes over time for both reactions.
Notes gb lab 07 chemical detective
The document discusses key concepts related to physical and chemical changes, including:
- The student will learn to distinguish between physical and chemical changes and understand chemical formulas and bond types.
- A physical change alters a substance's size, shape, or state but not its chemical makeup, while a chemical change produces a new substance.
- The Law of Conservation of Mass states that mass is neither created nor destroyed in a chemical reaction, though the substance and form may change.
- A chemical formula represents the elements in a compound using symbols, such as CO2 for carbon dioxide. A chemical equation models a reaction using formulas.
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Notes pb lab 06 part 2 the spectacular spectrum separating light
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Notes lab 04 ions and isotopes
- 2. Isotopes Atoms of the same element can have different numbers of neutrons; the different possible versions of the atom of an element are called isotopes Written as a symbol and a number i.e. C 14 is an isotope of carbon called Carbon 14
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