There are observable trends in the physical and chemical properties of elements across periods and down groups in the periodic table. As you move across a period, atomic radius decreases due to the increasing effective nuclear charge pulling the valence electrons closer. Down groups, atomic radius increases as each successive energy level is farther from the nucleus. Ionization energy generally increases across periods as effective nuclear charge increases, and decreases down groups as the valence electrons are farther from the nucleus. Electron affinity increases across periods but decreases down groups. Oxidation states can be used to keep track of electrons in compounds and ions.
In 1909, Rutherford performed the Gold Foil Experiment and suggested the following characteristics of the atom:
It consists of a small core, or nucleus, that contains most of the mass of the atom
This nucleus is made up of particles called protons, which have a positive charge
The protons are surrounded by negatively charged electrons, but most of the atom is actually empty space.
In 1913, Bohor proposed the Atomic Model, which suggests that electrons travel around the nucleus of an atom in orbits or definite paths.
Atom consists of a tiny nucleus.
Each orbit has fixed energy that is quantatized.
The energy is emitted or absorb only when an electron jumps from one orbit to another.
Electron can revolve in orbits of fixed angular momentum mvr.
Liquid Drop Model
The nuclei of all elements are considered to be behave like a liquid drop of incompressible liquid of very high density.
In an equilibrium state the nuclei of atoms remain spherically symmetric under the action of strong attractive nuclear forces just like the drop of a liquid which is spherical due to surface tension.
The density of a nucleus is independent of its
size just like the density of liquid which is also
independent of its size.
The protons and neutrons of the nucleus move about
within a spherical enclosure called the nuclear
potential barrier just like the movement of the
molecules of a liquid within a spherical drop of liquid.
. The binding energy per nucleon of a nucleus is constant
Binding Energy
The binding energy, BE, of a nucleus is a measure of the strong force and represents the energy required to separate the nucleus into its constituents protons and neutrons;
Greater the binding energy, the more stable the nucleus.
Volume
The volume of the nucleus is directly proportional to the total number of nucleons present in it.
Density
The density of the nucleus is nearly constant.
This PowerPoint is one small part of the Atoms and Periodic Table of the Elements unit from www.sciencepowerpoint.com. This unit consists of a five part 2000+ slide PowerPoint roadmap, 12 page bundled homework package, modified homework, detailed answer keys, 15 pages of unit notes for students who may require assistance, follow along worksheets, and many review games. The homework and lesson notes chronologically follow the PowerPoint slideshow. The answer keys and unit notes are great for support professionals. The activities and discussion questions in the slideshow are meaningful. The PowerPoint includes built-in instructions, visuals, and review questions. Also included are critical class notes (color coded red), project ideas, video links, and review games. This unit also includes four PowerPoint review games (110+ slides each with Answers), 38+ video links, lab handouts, activity sheets, rubrics, materials list, templates, guides, and much more. Also included is a 190 slide first day of school PowerPoint presentation.
Areas of Focus: -Atoms (Atomic Force Microscopes), Rutherford's Gold Foil Experiment, Cathode Tube, Atoms, Fundamental Particles, The Nucleus, Isotopes, AMU, Size of Atoms and Particles, Quarks, Recipe of the Universe, Atomic Theory, Atomic Symbols, #'s, Valence Electrons, Octet Rule, SPONCH Atoms, Molecules, Hydrocarbons (Structure), Alcohols (Structure), Proteins (Structure), Periodic Table of the Elements, Organization of Periodic Table, Transition Metals, Electron Negativity, Non-Metals, Metals, Metalloids, Atomic Bonds, Ionic Bonds, Covalent Bonds, Metallic Bonds, Ionization, and much more.
This unit aligns with the Next Generation Science Standards and with Common Core Standards for ELA and Literacy for Science and Technical Subjects. See preview for more information
If you have any questions please feel free to contact me. Thanks again and best wishes. Sincerely, Ryan Murphy M.Ed www.sciencepowerpoint@gmail.com
Teaching Duration = 4+ Weeks
This presentation has all the points covered under the heading of halogenoalkanes from the syllabus of AS Level Chemistry 2014-15 as alloted by Cambridge.
In 1909, Rutherford performed the Gold Foil Experiment and suggested the following characteristics of the atom:
It consists of a small core, or nucleus, that contains most of the mass of the atom
This nucleus is made up of particles called protons, which have a positive charge
The protons are surrounded by negatively charged electrons, but most of the atom is actually empty space.
In 1913, Bohor proposed the Atomic Model, which suggests that electrons travel around the nucleus of an atom in orbits or definite paths.
Atom consists of a tiny nucleus.
Each orbit has fixed energy that is quantatized.
The energy is emitted or absorb only when an electron jumps from one orbit to another.
Electron can revolve in orbits of fixed angular momentum mvr.
Liquid Drop Model
The nuclei of all elements are considered to be behave like a liquid drop of incompressible liquid of very high density.
In an equilibrium state the nuclei of atoms remain spherically symmetric under the action of strong attractive nuclear forces just like the drop of a liquid which is spherical due to surface tension.
The density of a nucleus is independent of its
size just like the density of liquid which is also
independent of its size.
The protons and neutrons of the nucleus move about
within a spherical enclosure called the nuclear
potential barrier just like the movement of the
molecules of a liquid within a spherical drop of liquid.
. The binding energy per nucleon of a nucleus is constant
Binding Energy
The binding energy, BE, of a nucleus is a measure of the strong force and represents the energy required to separate the nucleus into its constituents protons and neutrons;
Greater the binding energy, the more stable the nucleus.
Volume
The volume of the nucleus is directly proportional to the total number of nucleons present in it.
Density
The density of the nucleus is nearly constant.
This PowerPoint is one small part of the Atoms and Periodic Table of the Elements unit from www.sciencepowerpoint.com. This unit consists of a five part 2000+ slide PowerPoint roadmap, 12 page bundled homework package, modified homework, detailed answer keys, 15 pages of unit notes for students who may require assistance, follow along worksheets, and many review games. The homework and lesson notes chronologically follow the PowerPoint slideshow. The answer keys and unit notes are great for support professionals. The activities and discussion questions in the slideshow are meaningful. The PowerPoint includes built-in instructions, visuals, and review questions. Also included are critical class notes (color coded red), project ideas, video links, and review games. This unit also includes four PowerPoint review games (110+ slides each with Answers), 38+ video links, lab handouts, activity sheets, rubrics, materials list, templates, guides, and much more. Also included is a 190 slide first day of school PowerPoint presentation.
Areas of Focus: -Atoms (Atomic Force Microscopes), Rutherford's Gold Foil Experiment, Cathode Tube, Atoms, Fundamental Particles, The Nucleus, Isotopes, AMU, Size of Atoms and Particles, Quarks, Recipe of the Universe, Atomic Theory, Atomic Symbols, #'s, Valence Electrons, Octet Rule, SPONCH Atoms, Molecules, Hydrocarbons (Structure), Alcohols (Structure), Proteins (Structure), Periodic Table of the Elements, Organization of Periodic Table, Transition Metals, Electron Negativity, Non-Metals, Metals, Metalloids, Atomic Bonds, Ionic Bonds, Covalent Bonds, Metallic Bonds, Ionization, and much more.
This unit aligns with the Next Generation Science Standards and with Common Core Standards for ELA and Literacy for Science and Technical Subjects. See preview for more information
If you have any questions please feel free to contact me. Thanks again and best wishes. Sincerely, Ryan Murphy M.Ed www.sciencepowerpoint@gmail.com
Teaching Duration = 4+ Weeks
This presentation has all the points covered under the heading of halogenoalkanes from the syllabus of AS Level Chemistry 2014-15 as alloted by Cambridge.
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Welcome to UiPath Test Automation using UiPath Test Suite series part 4. In this session, we will cover Test Manager overview along with SAP heatmap.
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Orchestrator execution result
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Create a campaign using Mailchimp with merge tags/fields
Send an interactive Slack channel message (using buttons)
Have the message received by managers and peers along with a test email for review
But there’s more:
In a second workflow supporting the same use case, you’ll see:
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If the “Approve” button is clicked, a Jira/Zendesk ticket is created for the marketing design team
But—if the “Reject” button is pushed, colleagues will be alerted via Slack message
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After immersing yourself in the blue book and its red counterpart, attending DDD-focused conferences, and applying tactical patterns, you're left with a crucial question: How do I ensure my design is effective? Tactical patterns within Domain-Driven Design (DDD) serve as guiding principles for creating clear and manageable domain models. However, achieving success with these patterns requires additional guidance. Interestingly, we've observed that a set of constraints initially designed for training purposes remarkably aligns with effective pattern implementation, offering a more ‘mechanical’ approach. Let's explore together how Object Calisthenics can elevate the design of your tactical DDD patterns, offering concrete help for those venturing into DDD for the first time!
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2. PERIODIC TRENDS IN PROPERTIES
OF ELEMENTS
There are many observable patterns in the physical and chemical
properties of elements as we descend in a group or move across a
period in the Periodic Table.
We will rationalize observed trends in
Sizes of atoms and ions.
Ionization energy.
Electron affinity.
The bonding atomic
radius is defined as
one-half of the distance
between covalently
bonded nuclei.
The Size of an Atom
3. Trend in Atomic Radius
Different methods for measuring the radius of an atom, and
they give slightly different trends
Van der Waals radius = Nonbonding
Covalent radius = Bonding radius
Atomic radius is an average radius
of an atom based on measuring large
numbers of elements and compounds.
4. Valence shell farther from nucleus
Effective nuclear charge fairly close
Atomic Radius Decreases across period (left to right)
The number of energy levels increases as you move down a group as
the number of electrons increases. Each subsequent energy level is
further from the nucleus than the last. Therefore, the atomic radius
increases as the group and energy levels increase.
Atomic Radius Increases down group
Atomic Radius
adding electrons to same valence shell
effective nuclear charge increases
valence shell held closer
- As you go across a period, electrons are added to the same energy
level. At the same time, protons are being added to the nucleus. The
concentration of more protons in the nucleus creates a "higher
effective nuclear charge." In other words, there is a stronger force
of attraction pulling the electrons closer to the nucleus resulting in a
smaller atomic radius.
6. Sizes of Ions
• Ionic size depends upon
– The nuclear charge.
– The number of electrons.
– The orbital in which
electrons reside.
7. Sizes of Ions
• Cat ions are smaller than their parent atoms:
– The outermost electron is removed and repulsions between
electrons are reduced.
• Anions are larger than their parent atoms
– Electrons are added and repulsions between electrons are
increased.
• In an Isoelectronic series, ions have the same number
of electrons.
• Ionic size decreases with an increasing nuclear charge.
8. Ionization Energy
The ionization energy is the amount of energy
required to remove an electron from the ground state of
a gaseous atom or ion.
– The first ionization energy is that energy required to
remove the first electron.
– The second ionization energy is that energy
required to remove the second electron, etc.
• It requires more energy to remove each successive electron.
• When all valence electrons have been removed, the ionization
energy takes a quantum leap.
10. First Ionization Energies
Larger the effective nuclear charge on the electron,
the more energy it takes to remove it
The farther the most probable distance the electron is
from the nucleus, the less energy it takes to remove it
1st IE decreases down the group
valence electron farther from nucleus
1st IE generally increases across the period
effective nuclear charge increases
13. Irregularities in the Trend
Ionization Energy generally increases from left to
right across a Period
except from 2A to 3A, 5A to 6A
Be
1s 2s 2p
B
1s 2s 2p
N
1s 2s 2p
O
1s 2s 2p
Which is easier to remove an
electron from B or Be? Why?
Which is easier to remove an
electron from N or O? Why?
14. Irregularities in the
First Ionization Energy Trends
Be
1s 2s 2p
B
1s 2s 2p
Be+
1s 2s 2p
To ionize Be you must break up a full sublevel, cost extra energy
B+
1s 2s 2p
When you ionize B you get a full sublevel, costs less energy
15. Irregularities in the
First Ionization Energy Trends
To ionize N you must break up a half-full sublevel, cost extra energy
N+
1s 2s 2p
O
1s 2s 2p
N
1s 2s 2p
O+
1s 2s 2p
When you ionize O you get a half-full sublevel, costs less energy
16. Trends in Successive
Ionization Energies
Removal of each successive electron
costs more energy
– shrinkage in size due to having more
protons than electrons
– outer electrons closer to the nucleus,
therefore harder to remove
Regular increase in energy for each
successive valence electron
Rarge increase in energy when start
removing core electrons
18. Electron Affinity
Electron affinity is the energy change accompanying
the addition of an electron to a gaseous atom:
Cl + e− Cl−
1) As you move down a group, electron affinity decreases.
2) As you move across a period, electron affinity increases.
19. Electron Affinity
The first occurs between
Groups IA and IIA.
– The added electron must go in a
p orbital, not an s orbital.
– The electron is farther from the
nucleus and feels repulsion from
the s electrons.
The second discontinuity
occurs between Groups IVA
and VA.
– Group VA has no empty
orbitals.
– The extra electron must go into
an already occupied orbital,
creating repulsion.
20. Oxidation States
A way of keeping track of the electrons.
Not necessarily true of what is in nature, but it works.
need the rules for assigning .
The oxidation state of elements in their standard states is zero.
Oxidation state for monatomic ions are the same as their charge.
Oxygen is assigned an oxidation state of -2 in its covalent
compounds except as a peroxide.
In compounds with nonmetals hydrogen is assigned the oxidation
state +1.
In its compounds fluorine is always –1.
The sum of the oxidation states must be zero in compounds or
equal the charge of the ion.
21. Oxidation States
1. The oxidation state of any element such as Fe, H2, O2, P4,
S8 is zero (0).
2. The oxidation state of oxygen in its compounds is -2, except
for peroxides like H2O2, and Na2O2, in which the oxidation
state for O is -1.
3. The oxidation state of hydrogen is +1 in its compounds,
except for metal hydrides, such as NaH, LiH, etc., in which
the oxidation state for H is -1.
4. The oxidation states of other elements are then assigned to
make the algebraic sum of the oxidation states equal to the
net charge on the molecule or ion.
5. The following elements usually have the same oxidation
states in their compounds:+1 for alkali metals - Li, Na, K, Rb,
Cs;
6. +2 for alkaline earth metals - Be, Mg, Ca, Sr, Ba;
7. -1 for halogens except when they form compounds with
oxygen or one another;
22. Element
Oxidation
state
Compound
or ion
Fe +2 Fe2+ Fe = Fe2+ + 2 e-
+3 Fe3+ Fe2+ = Fe3++ e-
Zn 0 Zn Zn is reducing agent
+2 Zn2+
O -1 H2O2 H2O2 = O2 + H2O
0 O2
-2 H2O
Oxidation States
23. The End
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