This document discusses natural radioactivity and the different types of natural nuclear transmutations that can occur. It explains that larger atoms are generally more unstable due to having a greater proton to neutron ratio further from 1:1. The three main types of natural transmutations discussed are alpha decay, beta decay, and gamma decay. Alpha decay involves emitting an alpha particle, beta decay involves emitting an electron or positron, and gamma decay involves emitting high energy photons without any particle emission. Examples of writing nuclear reactions are provided to identify the missing particle.
This document discusses graphing square root functions, with 6 examples provided of graphing different square root functions by plotting points and sketching the graphed curve. The section number, topic of graphing square root functions, and a statement that 6 examples will be provided are given.
Discovering DNA
- In the mid-1800s it was known that cells contained nuclei with large molecules called nucleic acids, but the arrangement was still unknown in the 1950s.
- Rosalind Franklin discovered that DNA is a double helix of two spiraling chains of molecules.
- Watson and Crick further studied the DNA model and discovered that each side is made of a sugar-phosphate molecule and the rungs are made of nitrogen bases that always pair the same way.
Genes
- Genes are sections of DNA that contain instructions for making proteins. Chromosomes contain many genes. The gene code determines the order of amino acids that link to form a protein. RNA carries the gene code out
Bulletproof presented our services and story to the Calgary Chamber of Commerce. We covered the importance of having a trusted IT business adviser and how we serve the business community of Calgary and Red Deer
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 bond: by losing electrons, gaining electrons, pooling electrons, and sharing electrons. It then focuses on bonding by losing and gaining electrons using sodium and chlorine as examples. Sodium loses an electron to become stable, giving it a positive charge, while chlorine gains an electron to become stable, giving it a negative charge.
Atoms bond together by sharing or transferring valence electrons. Valence electrons are found in the outermost energy level of an atom and participate in chemical bonding. The number of valence electrons an atom has determines how many bonds it can form. Atoms are most stable when they have eight valence electrons, as this full outer energy level is very unlikely to react. Atoms with fewer than eight valence electrons seek to gain or share electrons through bonding in order to achieve a stable electron configuration.
Ch.2 the structure of matter and the chemical elementsKeith James
This document provides an overview of models and the structure of matter. It discusses how models are simplified representations of reality used in science, architecture, and business. Matter is composed of tiny particles that are in constant motion. The motion of particles is related to temperature and the state of matter. Solids, liquids, and gases differ in how freely particles can move and how strongly they attract each other. Elements are the fundamental units that make up compounds and cannot be broken down further chemically. The periodic table organizes elements according to their properties and atomic structure. Elements can have different isotopes that vary in neutron number. Molecules form when atoms bond together via sharing or exchanging electrons.
Blood transports oxygen, nutrients, hormones, carbon dioxide, and waste throughout the body. It also fights infections through white blood cells and helps regulate temperature. Blood is made up of plasma, platelets, red blood cells, and white blood cells. It exists in different blood types (A, B, AB, O) and Rh factors (+ or -) to prevent incompatible mixing. Diseases can affect blood cells like leukemia and anemia.
Molecular gastronomy is a subdiscipline of food science that investigates the physical and chemical transformations of ingredients during cooking. It was coined in 1992 by Hungarian physicist Nicholas Kurti and French chemist Hervé This. Molecular gastronomy uses techniques like spherification, gelification, thickening, and emulsification to transform foods using additives like sodium alginate, calcium salts, agar-agar, and soy lecithin. These techniques allow chefs to deconstruct and reconstruct dishes in new forms. Molecular gastronomy has the potential to make significant contributions to cuisine in the future.
This document discusses graphing square root functions, with 6 examples provided of graphing different square root functions by plotting points and sketching the graphed curve. The section number, topic of graphing square root functions, and a statement that 6 examples will be provided are given.
Discovering DNA
- In the mid-1800s it was known that cells contained nuclei with large molecules called nucleic acids, but the arrangement was still unknown in the 1950s.
- Rosalind Franklin discovered that DNA is a double helix of two spiraling chains of molecules.
- Watson and Crick further studied the DNA model and discovered that each side is made of a sugar-phosphate molecule and the rungs are made of nitrogen bases that always pair the same way.
Genes
- Genes are sections of DNA that contain instructions for making proteins. Chromosomes contain many genes. The gene code determines the order of amino acids that link to form a protein. RNA carries the gene code out
Bulletproof presented our services and story to the Calgary Chamber of Commerce. We covered the importance of having a trusted IT business adviser and how we serve the business community of Calgary and Red Deer
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 bond: by losing electrons, gaining electrons, pooling electrons, and sharing electrons. It then focuses on bonding by losing and gaining electrons using sodium and chlorine as examples. Sodium loses an electron to become stable, giving it a positive charge, while chlorine gains an electron to become stable, giving it a negative charge.
Atoms bond together by sharing or transferring valence electrons. Valence electrons are found in the outermost energy level of an atom and participate in chemical bonding. The number of valence electrons an atom has determines how many bonds it can form. Atoms are most stable when they have eight valence electrons, as this full outer energy level is very unlikely to react. Atoms with fewer than eight valence electrons seek to gain or share electrons through bonding in order to achieve a stable electron configuration.
Ch.2 the structure of matter and the chemical elementsKeith James
This document provides an overview of models and the structure of matter. It discusses how models are simplified representations of reality used in science, architecture, and business. Matter is composed of tiny particles that are in constant motion. The motion of particles is related to temperature and the state of matter. Solids, liquids, and gases differ in how freely particles can move and how strongly they attract each other. Elements are the fundamental units that make up compounds and cannot be broken down further chemically. The periodic table organizes elements according to their properties and atomic structure. Elements can have different isotopes that vary in neutron number. Molecules form when atoms bond together via sharing or exchanging electrons.
Blood transports oxygen, nutrients, hormones, carbon dioxide, and waste throughout the body. It also fights infections through white blood cells and helps regulate temperature. Blood is made up of plasma, platelets, red blood cells, and white blood cells. It exists in different blood types (A, B, AB, O) and Rh factors (+ or -) to prevent incompatible mixing. Diseases can affect blood cells like leukemia and anemia.
Molecular gastronomy is a subdiscipline of food science that investigates the physical and chemical transformations of ingredients during cooking. It was coined in 1992 by Hungarian physicist Nicholas Kurti and French chemist Hervé This. Molecular gastronomy uses techniques like spherification, gelification, thickening, and emulsification to transform foods using additives like sodium alginate, calcium salts, agar-agar, and soy lecithin. These techniques allow chefs to deconstruct and reconstruct dishes in new forms. Molecular gastronomy has the potential to make significant contributions to cuisine in the future.
The document discusses radioactivity, which is the spontaneous emission of particles or radiation from radioactive substances. It explains that there are three types of rays - alpha, beta, and gamma rays - produced by the decay or breakdown of radioactive materials, and each type is affected differently by electric or magnetic fields. The penetrating abilities of the different types of rays through materials like lead is also illustrated.
Here are the steps to solve a half-life problem:
1. Pick a starting mass (e.g. 30 g)
2. Choose a half-life (e.g. 5 years)
3. Plot the mass after each half-life on a graph with mass on the y-axis and time/half-lives on the x-axis
4. The graph will be exponential decay
5. Mass never reaches exactly zero
6. Radioactivity is no longer a problem after about 5-7 half-lives as the mass becomes very small
7. Exponential decay is described by the equation: M = M0 * (1/2)^(t/t1/2)
This document provides information about nuclear chemistry and radioactivity. It discusses isotopes and how they differ in the number of neutrons while having the same number of protons. It explains how isotopes are denoted and how to determine the number of protons, neutrons, and electrons for different isotopes. The document also describes the three types of radiation emitted by radioactive isotopes - alpha, beta, and gamma radiation - and their properties. It discusses radioactive decay processes like alpha decay, beta decay, and gamma decay. Key concepts like half-life and nuclear fission are summarized. Nuclear chemistry concepts are illustrated through examples and diagrams.
The document discusses radioactive decay and how the nucleus changes during this process. It explains that radioactive decay occurs when an unstable parent isotope emits an alpha, beta, or gamma particle, transforming into a stable daughter product. The document provides examples of using atomic number and mass to identify daughter products from parent isotopes undergoing alpha or beta decay.
Radioactive decay involves the spontaneous breakdown of an unstable nucleus through alpha, beta, or gamma decay. Alpha decay involves emitting an alpha particle (helium nucleus), beta decay involves emitting an electron, and gamma decay involves emitting electromagnetic radiation. Balancing nuclear equations requires that the sums of atomic numbers and mass numbers are equal on both sides of the equation. Artificial transmutation through particle bombardment can produce nuclei with different numbers of protons and neutrons compared to the original.
Nuclear chemistry documents the three main types of radioactive decay - alpha, beta, and gamma - and how the nucleus changes in each. It also explains that alpha, beta, and gamma radiation produce different levels of tissue damage and penetration. Naturally occurring and artificially produced isotopes can be radioactive. Nuclear fission and fusion reactions release much more energy per gram than chemical reactions, with a small but significant mass change accounted for by Einstein's equation relating energy and mass.
Alpha decay occurs when an unstable atom emits an alpha particle, which is a helium nucleus containing 2 protons and 2 neutrons, becoming a more stable atom. Beta decay is when a neutron changes into a proton and electron, increasing the atomic number by 1 but keeping the mass number the same. Gamma decay releases excess energy from an atom as electromagnetic gamma ray photons after alpha or beta decay.
Radioactive decay occurs through three main types: alpha decay, beta decay, and gamma decay. Alpha decay involves emitting an alpha particle, which is identical to a helium nucleus containing two protons and two neutrons. Beta decay results in one less neutron but one extra proton. Gamma decay occurs when atoms are still energetic after alpha or beta decay and emit gamma rays to become stable. These decays are important applications in areas like nuclear medicine, nuclear reactors, and sterilization.
1. Nuclear reactions involve changes within the nucleus, releasing radiation such as alpha particles, beta particles, or positrons.
2. Common types of nuclear decay include alpha decay, which releases an alpha particle; beta decay, which releases beta particles or positrons; and positron emission, which releases positrons.
3. Nuclear decay can be used to identify different forms of radiation and predict products of nuclear reactions based on balancing nuclear equations. The rate of decay is characterized by an isotope's half-life.
This document discusses radioactivity and nuclear decay. It describes Henri Becquerel's 1899 discovery of radioactivity by accidently exposing photographic plates to uranium salts. It then covers the different types of nuclear decay including alpha, beta, and gamma decay. Examples of specific radioactive elements that undergo each type of decay are given, such as americium-241 undergoing alpha decay. Symbols used to represent subatomic particles like electrons, positrons, neutrons, and protons in nuclear reactions are also defined.
The document discusses radioactivity, which is the spontaneous emission of particles or radiation from radioactive substances. It explains that there are three types of rays - alpha, beta, and gamma rays - produced by the decay or breakdown of radioactive materials, and each type is affected differently by electric or magnetic fields. The penetrating abilities of the different types of rays through materials like lead is also illustrated.
Here are the steps to solve a half-life problem:
1. Pick a starting mass (e.g. 30 g)
2. Choose a half-life (e.g. 5 years)
3. Plot the mass after each half-life on a graph with mass on the y-axis and time/half-lives on the x-axis
4. The graph will be exponential decay
5. Mass never reaches exactly zero
6. Radioactivity is no longer a problem after about 5-7 half-lives as the mass becomes very small
7. Exponential decay is described by the equation: M = M0 * (1/2)^(t/t1/2)
This document provides information about nuclear chemistry and radioactivity. It discusses isotopes and how they differ in the number of neutrons while having the same number of protons. It explains how isotopes are denoted and how to determine the number of protons, neutrons, and electrons for different isotopes. The document also describes the three types of radiation emitted by radioactive isotopes - alpha, beta, and gamma radiation - and their properties. It discusses radioactive decay processes like alpha decay, beta decay, and gamma decay. Key concepts like half-life and nuclear fission are summarized. Nuclear chemistry concepts are illustrated through examples and diagrams.
The document discusses radioactive decay and how the nucleus changes during this process. It explains that radioactive decay occurs when an unstable parent isotope emits an alpha, beta, or gamma particle, transforming into a stable daughter product. The document provides examples of using atomic number and mass to identify daughter products from parent isotopes undergoing alpha or beta decay.
Radioactive decay involves the spontaneous breakdown of an unstable nucleus through alpha, beta, or gamma decay. Alpha decay involves emitting an alpha particle (helium nucleus), beta decay involves emitting an electron, and gamma decay involves emitting electromagnetic radiation. Balancing nuclear equations requires that the sums of atomic numbers and mass numbers are equal on both sides of the equation. Artificial transmutation through particle bombardment can produce nuclei with different numbers of protons and neutrons compared to the original.
Nuclear chemistry documents the three main types of radioactive decay - alpha, beta, and gamma - and how the nucleus changes in each. It also explains that alpha, beta, and gamma radiation produce different levels of tissue damage and penetration. Naturally occurring and artificially produced isotopes can be radioactive. Nuclear fission and fusion reactions release much more energy per gram than chemical reactions, with a small but significant mass change accounted for by Einstein's equation relating energy and mass.
Alpha decay occurs when an unstable atom emits an alpha particle, which is a helium nucleus containing 2 protons and 2 neutrons, becoming a more stable atom. Beta decay is when a neutron changes into a proton and electron, increasing the atomic number by 1 but keeping the mass number the same. Gamma decay releases excess energy from an atom as electromagnetic gamma ray photons after alpha or beta decay.
Radioactive decay occurs through three main types: alpha decay, beta decay, and gamma decay. Alpha decay involves emitting an alpha particle, which is identical to a helium nucleus containing two protons and two neutrons. Beta decay results in one less neutron but one extra proton. Gamma decay occurs when atoms are still energetic after alpha or beta decay and emit gamma rays to become stable. These decays are important applications in areas like nuclear medicine, nuclear reactors, and sterilization.
1. Nuclear reactions involve changes within the nucleus, releasing radiation such as alpha particles, beta particles, or positrons.
2. Common types of nuclear decay include alpha decay, which releases an alpha particle; beta decay, which releases beta particles or positrons; and positron emission, which releases positrons.
3. Nuclear decay can be used to identify different forms of radiation and predict products of nuclear reactions based on balancing nuclear equations. The rate of decay is characterized by an isotope's half-life.
This document discusses radioactivity and nuclear decay. It describes Henri Becquerel's 1899 discovery of radioactivity by accidently exposing photographic plates to uranium salts. It then covers the different types of nuclear decay including alpha, beta, and gamma decay. Examples of specific radioactive elements that undergo each type of decay are given, such as americium-241 undergoing alpha decay. Symbols used to represent subatomic particles like electrons, positrons, neutrons, and protons in nuclear reactions are also defined.
1. A. Natural Radioactivity
Many nuclei of atoms are very stable, others are
unstable and will decay
Based on the ratio of protons to neutrons
Further from a 1:1 ratio, more likely to decay
12 C 6 protons, 6 neutrons stable
6
13 C 6 protons, 7 neutrons unstable
6
Larger atoms are generally more unstable
No stable isotopes past Bi All are radioactive
2. Natural Transmutation Atom releases energy (usually as a
particle) and transforms into a different element
C
14
N
14
The nucleus breaks down with no outside interference (natural)
A. Types of Natural Transmutations
1. Alpha Decay α
Releases an alpha particle 2 protons and 2 neutrons
Written as 4 He Same as a Helium nucleus
2
Low energy particle
Little ionizing power Cannot break apart molecules well
Low penetrating ability, blocked by paper
3. 2. Beta particle β
- Releases a beta particle and energy from the nucleus
- Actually it is an electron
0 No noticeable mass
Opposite charge of a proton
e
-1
- a neutron breaks down into an electron and a proton
- the electron is then released from the nucleus
Moves faster than alpha, almost to the speed of light
More damaging, - Higher penetrating ability and ionizing
ability blocked by thin sheets of lead
3. Gamma decay γ
No particle, just a release of energy
Energy is similar to high energy x-rays
Very high ionizing ability and penetrating ability
Can penetrate several cm of lead, blocked by thick lead
4.
5. Chart N - Lists types of decays for many nuclei
B. Writing Nuclear Reactions
We can determine what particles are present by what is
left after the decay 222
Rn
86
86
226
Ra --> 4 He + _________
88 2
Since we lost 4 nuclear particles We have 222 left
Since we lost 2 protons We have 86 left
To determine the identity, look at the atomic number
and match it to the periodic table
6.
7. Examples - Determine the missing nuclear particle
210
Bi
A. 210Pb --> ______ + 0e beta
82
83 -1
0
B. 214
Bi --> 214
Po + _______
e beta
4 -1
83 84
He
C. 214Po --> _________ + Pb
210 alpha
2
206
D. 206Tl -->
84
0
e + ________
Pb 82 beta
82
Now 81 back-1and label the reactions as alpha or beta decay
go
Use chart N to determine the products of the following
A.
85
Kr 0
e + 85 Rb Beta decay
36 -1
37
B. 232
Th 4
He +
228
Ra Alpha decay
88
2
90