Isoto dotdiag predreact
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Lithium will try to lose its 1 valence electron since that is the least amount of work. It is most likely to bond with fluorine since fluorine needs 1 extra electron to be stable. After bonding, lithium will have a +1 charge and fluorine will have a -1 charge.
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Isotopes, Lewis Dot Diagrams and Predicting Reactions
This document provides a review of key concepts related to isotopes, Lewis dot diagrams, and predicting chemical reactions. It defines isotopes as variants of the same element with different numbers of neutrons. Lewis dot diagrams represent valence electrons and allow prediction of how atoms will react to gain or lose electrons to achieve stable full outer shells like noble gases. Atoms react in the simplest way possible to satisfy this rule by losing or gaining the fewest electrons.
Difference between an Ion and a Radical
"Ions are any atoms or molecules that have a net charge. Hence an ion is any discrete molecular substance where the number of protons and the number of electrons are different".
"Radicals are formed when an orbital has an unpaired electron". Radicals have an odd number of electrons, meaning at least one electron is in an orbital by itself, unpaired”.
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This document discusses valence electrons and how to determine the number available for bonding using the periodic table. It defines valence electrons as those in the outermost shell or energy level available for bonding. It provides examples of how many valence electrons elements in different groups have, from 1 to 8. It also introduces Lewis dot structures as a way to represent an atom's valence electrons and provides examples of Lewis dot structures for period 2 elements.
Valence and lewis dot structure
Here are the Lewis electron dot diagrams for the requested elements and ions:
1.
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How to-bohr-diagram
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"Ions are any atoms or molecules that have a net charge. Hence an ion is any discrete molecular substance where the number of protons and the number of electrons are different".
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Isotopes have the same number of protons but different numbers of neutrons. Writing an isotope without the atomic number, like 35S, indicates that it is an isotope of the element with atomic number 16 (sulfur). The atomic number is omitted because it is implied by the element symbol.
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2. Draw an initial sketch showing the atoms. Place each atom's valence electrons around it.
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An atom is composed of a nucleus containing protons and neutrons surrounded by electrons. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons exist outside the nucleus in the electron cloud. The number of protons defines the element and is equal to the atomic number. The total number of protons and neutrons is the mass number. For neutral atoms, the number of electrons equals the number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
11/16/11
The charge of the ion is indicated
by the superscript number after the element
symbol. A positive number means the atom
lost electrons and is positively charged. A
negative number means the atom gained
electrons and is negatively charged.
Model: Na+ Ion
Sodium ion (Na) that lost 1 electron
Charge: +1
Protons: 11
Electrons: 10
Neutrons: 12
Mass: 22.9898
Model this ion in your notebook!
Model: Cl- Ion
Chlorine ion (Cl) that gained 1 electron
Charge: -1
Protons: 17
Electrons: 18
Neutrons: 18
Atoms elements
Atoms and elements can combine in many ways to form useful compounds. An element is made of identical atoms, while a compound is formed from two or more elements chemically bonded together. Atoms are the simplest form of an element, with protons and neutrons in the nucleus and electrons orbiting around. The number of protons determines the element, while isotopes of an element differ in their number of neutrons. Electrons are usually contained within atoms but can give electric shocks. Atoms combine in fixed ratios to form molecules, with the molecular mass determined by adding the atomic masses. Large numbers of atoms are measured in moles, with one mole equaling 6.02x1023 units. Elements form ions by gaining or losing
General Biology. LECTURE 2. THE CHEMICAL FOUNDATION OF LIFE.pptx
This document provides an overview of the chemical foundations of life. It discusses that biochemistry is the study of the structures and roles of chemicals in living organisms. The key points made are:
- Life depends on chemistry as living things are composed of chemical elements like carbon, hydrogen, oxygen, nitrogen.
- Atoms are the basic unit of matter and combine to form molecules and chemical compounds. The four most common elements in living things are carbon, hydrogen, oxygen, and nitrogen.
- Isotopes are atoms of the same element that vary in neutron number. There are three isotopes of hydrogen: protium, deuterium, and tritium.
The_Atom.ppt
1) The atomic model has evolved over time as new evidence and theories emerged. Early models included the plum pudding model and Rutherford's model of a small, dense nucleus surrounded by electrons.
2) Bohr's model improved on this by proposing that electrons orbit the nucleus in fixed, quantized energy levels. Electrons absorb or emit photons of specific energies when changing levels.
3) Later, the wave mechanical model described electrons as existing in orbital regions rather than fixed orbits, depicted as electron clouds or probability distributions. This provides a more accurate quantum mechanical description of electrons in atoms.
The_Atom.ppt science 8 quarter 3 module 5
1) Models of the atom have evolved over time as new evidence and theories emerged. Early models included Thomson's "plum pudding" model and Rutherford's nuclear model.
2) Bohr's model improved on earlier work by proposing that electrons orbit the nucleus in fixed, quantized energy levels.
3) Later, the wave mechanical model described electrons as existing in orbitals or regions of probability rather than distinct orbits, better explaining experimental observations.
Intro to atoms (edited for 2016)
You could cut a gold bar in half forever, getting smaller pieces, but you would eventually reach the smallest possible piece that is still gold - the atom. An atom is the smallest particle of an element that retains the properties of that element. Atoms are made up of protons, neutrons, and electrons. The number of protons determines what element the atom is.
The atom
The document summarizes key information about atoms and their structure. It discusses:
- Atoms as the smallest part of an element, composed of subatomic particles
- The three main subatomic particles: protons, neutrons, and electrons, including their relative charge and mass
- Atoms containing all the element's protons and neutrons in the nucleus, with electrons in shells surrounding the nucleus
- The atomic number representing the number of protons in an atom, which also equals the number of electrons
- Carbon as an example, with an atomic number of 6 and electron configuration of 2 electrons in the first shell and 4 in the second
- The outer electron shell corresponding to the element's group
Valence electrons and lewis dot
Visiting a volcano would be the better class field trip for three reasons:
1) Volcanoes demonstrate geological processes like lava flows and eruptions that help students learn earth science.
2) Seeing volcanic landscapes up close helps students understand how volcanoes shape the environment.
3) Volcanoes present hazards but are also sites of new land being formed, offering learning opportunities about geological cycles.
How to draw Bohr diagrams
The document provides instructions for drawing Bohr diagrams to represent atomic structure:
1) Find the element on the periodic table to determine the number of protons and electrons, which is equal to the atomic number.
2) Draw the nucleus and electron shells based on the element's period - the number of shells equals the period number.
3) Add electrons to each shell following the rules that the first shell holds 2 electrons and subsequent shells hold up to 8 electrons, representing the subatomic particle composition of the element.
Periodic Trends Complete.ppt
1. Dimitri Mendeleev was the first to publish an organized periodic table and predicted the properties of undiscovered elements.
2. Henry Moseley later arranged the periodic table by atomic number, which is the modern version.
3. The periodic law states that when elements are arranged by atomic number, they display a repeating pattern of chemical and physical properties.
10/15 Review: Atomic Structure
This document provides an overview of an upcoming chemistry class covering atomic structure. The weekly schedule outlines topics to be covered each day, including atomic radius, electronegativity, atomic structure, and a midterm exam on Friday. Students are instructed to sketch the periodic table and label families for homework. The document then reviews atomic structure, including the dense nucleus at the center containing protons and neutrons, and less dense electron shells. Examples are given to calculate protons, neutrons, and electrons in different atoms. Homework assigned is to make a study notecard and complete a review worksheet in preparation for the midterm.
Similar to Isoto dotdiag predreact (20)
General Biology. LECTURE 2. THE CHEMICAL FOUNDATION OF LIFE.pptx
General Biology. LECTURE 2. THE CHEMICAL FOUNDATION OF LIFE.pptx
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Isoto dotdiag predreact
- 1. Isotopes Lewis dot diagrams and predicting reactions
- 2. But First, Let’s Review!! • Name the three • Protons, neutrons, subatomic particles electrons that an atom is made of.
- 3. But First, Let’s Review!! • How do I calculate the • It’s the same as the number of protons? atomic number!
- 4. But First, Let’s Review!! • How do I know how • Round the atomic many neutrons there mass and subtract the are? atomic number!
- 5. But First, Let’s Review!! • How do I know how • It’s the same as the many electrons there number of protons! are? That’s how the charge of the atom stays neutral!
- 6. But First, Let’s Review!! • Where does most of • The nucleus and it the atoms mass come consists of protons from? AND what and neutrons! subatomic particles does it include?
- 7. But First, Let’s Review!! • How many electrons • 2, 8, 8 are on the first, second an third shell?
- 8. But First, Let’s Review!! • Who can draw a Bohr diagram for Sulfur?
- 9. Great Job! NOW we can learn more stuff!
- 10. Isotopes • Isotopes are another type of atom of the same chemical element with more neutrons. • An isotope of Carbon, is still carbon it just has more neutrons in the nucleus. • Having more neutrons does not affect the atomic number because the number of protons stays the same.
- 11. Isotopes • Some isotopes are radioactive while most are quite stable. • C14 is a radioactive form of Carbon, where C12 and C13 are stable isotopes. • C14 still has 6 protons (because the atomic number has not changed) but has 8 neutrons instead of 6.
- 12. Lewis dot Diagrams • When predicting reactions, valence electrons are very important!!! • Valence electrons- electrons that are on the outermost shell. • Lewis dot diagrams are similar to Bohr Diagrams but they only show the outermost shell.
- 13. Lewis dot Diagrams • Bohr Diagram: • Lewis dot Diagram: F F
- 14. Lewis dot Diagrams • This diagram allows us to focus only on the valence electrons- which is all we really care about when predicting reactions.
- 15. Lewis dot Diagrams • One more short-cut: Rather than have to draw a Bohr diagram first, or do the math to figure out the number of valence electrons- all you need to do is look at the number at the top of the column. • EX: Phosphorus is in group 17, so it has 7 valence electrons. • EX: Carbon is in group 14, it has 4 valence electrons • EX: Hydrogen is in group 1, it has 1 valence electron
- 16. Predicting Reactions • RULE 1: Everyone wants to be a noble gas!! The noble gasses are PERFECT. They have a full outer shell. All elements want to have a full outer shell. • RULE 2: No one plays unless everyone is happy. All elements reacting must get what they want or no one reacts.
- 17. Predicting Reactions • If I have Beryllium and Oxygen, how many atoms of each will I need to satisfy both rules? • Beryllium has 2 valence electrons that it wants to get rid of. • Oxygen has 6 valence electrons and needs to gain 2.
- 18. Predicting Reactions Be O We only need one of each! Beryllium is happy because it lost the two outer electrons, and went to its inner full shell. Oxygen is happy because with Berylliums two electrons it now has a full outer shell!
- 19. Predicting Reactions • Atoms are lazy (like you!) and they don’t want to do too much work. If they only need to lose 1,2, or 3 electrons, they will do that rather than search for 5,6, or 7 to fill their shell. • Atoms will do the least amount of work to gain or lose electrons in order to have a full outer shell. • Remember 2 on the first shell is full! ! !
- 20. Predicting Reactions: Lithium • Lithium is atomic number 3 • How many protons does Lithium have? • How many Neutrons does it have? • How many electrons does it have? • How many valence electrons does it have? (What group is it in?) • What would a Bohr Diagram look like for Lithium?
- 21. Predicting Reactions: Lithium • Will lithium try to lose it’s 1 electron? Or will it try to find 7? Which is easier? • Who is it lost likely to bond with? Who needs to find an extra electron in order to be happy? • What will the charge of it be in the end?