Notes lab 04c ions and isotopes
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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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Notes lab 04 ions and isotopes
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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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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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.
Source
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.
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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This document provides information about atomic structure:
1) Atoms contain a nucleus with protons and neutrons at the center, surrounded by electrons in shells.
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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Notes lab 04 ions and isotopes
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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Source
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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2) The nucleus contains an equal number of protons and electrons, giving the atom a neutral charge.
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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 04c 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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