The document summarizes key concepts about the periodic table including periods, groups, and blocks. It explains that periods are horizontal rows based on the same principal quantum number, while groups are vertical columns with the same number of valence electrons. Blocks refer to different regions (s, p, d, f) based on which orbitals are being filled with electrons. It provides examples of trends in ionization energy and atomic radius across periods and down groups.
This is an effort to make ppt of p block elements , a topic in XII, chemistry(cbse) , whom as a tutor i have often felt students are horrified due to its large text size, long descriptipns, several information to be remembered and several reasonings to keep in mind.
Hope this ppt would solve thier problem of a thorough preparation of topic with all important aspects covered in the ppt.
Founder Dr Mona Srivastava
Masterchemclasses
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
This is an effort to make ppt of p block elements , a topic in XII, chemistry(cbse) , whom as a tutor i have often felt students are horrified due to its large text size, long descriptipns, several information to be remembered and several reasonings to keep in mind.
Hope this ppt would solve thier problem of a thorough preparation of topic with all important aspects covered in the ppt.
Founder Dr Mona Srivastava
Masterchemclasses
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
This is a presentation file that will provide you notes, proper diagrams, short tips, mnemonics about the alkali metals.. This course is of High School of grades 11 and 12. I think it will help every type of student. Similarly, you can find some repeated and important questions.
This is a presentation file that will provide you notes, proper diagrams, short tips, mnemonics about the alkali metals.. This course is of High School of grades 11 and 12. I think it will help every type of student. Similarly, you can find some repeated and important questions.
How to Make a Field invisible in Odoo 17Celine George
It is possible to hide or invisible some fields in odoo. Commonly using “invisible” attribute in the field definition to invisible the fields. This slide will show how to make a field invisible in odoo 17.
A Strategic Approach: GenAI in EducationPeter Windle
Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
Honest Reviews of Tim Han LMA Course Program.pptxtimhan337
Personal development courses are widely available today, with each one promising life-changing outcomes. Tim Han’s Life Mastery Achievers (LMA) Course has drawn a lot of interest. In addition to offering my frank assessment of Success Insider’s LMA Course, this piece examines the course’s effects via a variety of Tim Han LMA course reviews and Success Insider comments.
Model Attribute Check Company Auto PropertyCeline George
In Odoo, the multi-company feature allows you to manage multiple companies within a single Odoo database instance. Each company can have its own configurations while still sharing common resources such as products, customers, and suppliers.
Acetabularia Information For Class 9 .docxvaibhavrinwa19
Acetabularia acetabulum is a single-celled green alga that in its vegetative state is morphologically differentiated into a basal rhizoid and an axially elongated stalk, which bears whorls of branching hairs. The single diploid nucleus resides in the rhizoid.
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...
IB Chemistry on Periodic Trends, Effective Nuclear Charge and Physical properties.
1. Periodic Table of elements – divided to Groups, Periods and Blocks
Period- Horizontal row
• 7 periods/row
• Same number of shell
Groups – Vertical column
• Same number of valence electron
• Same number outmost electrons
Group 1
Block – different region in periodic table
• s, p, d, f blocks
• s block- elements with valence e in s sublevel
• p block – elements with valence e in p sublevel
18
Periods
1
7
Excellent site from periodic videos
Click here to view
s block
- s orbitals partially fill
d block
• d orbitals partially fill
p block
• p orbital partially fill
f block
• f orbital partially fill
2. s block elements
• s orbitals partially fill
1
H
He
p block elements
• p orbital partially fill
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
Periodic Table – s, p d, f blocks elements
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
20
K
Ca
[Ne] 3s2 3p2
[Ar]
15
P
[Ne] 3s2 3p3
[Ar]
4s2
16
S
[Ne] 3s2 3p4
17
19
Si
4s1
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
d block elements
• d orbitals partially fill
• transition elements
21
Sc
[Ar] 4s2 3d1
22
Ti
[Ar] 4s2 3d2
23
V
[Ar] 4s2 3d13
24
Cr
[Ar] 4s1 3d5
25
Mn
[Ar] 4s2 3d5
26
Fe
[Ar] 4s2 3d6
27
Co
[Ar] 4s2 3d7
28
Ni
[Ar] 4s2 3d8
29
Cu
[Ar] 4s1 3d10
30
Zn
[Ar] 4s2 3d10
f block elements
• f orbitals partially fill
Video on electron configuration
Click here electron structure
Click here video on s,p,d,f notation
Click here video s,p,d,f blocks,
3. Periodicity
Predicted pattern/trends in physical/chemical properties across period.
Physical properties
Chemical properties
Physical change - without change in molecular composition.
– appearance change
- composition remain unchanged.
Element properties
•
•
•
•
•
Atomic properties
•
•
•
•
Color, texture, odor
Density, hardness, ductility
Brittleness, Malleability
Melting /boiling point
Solubility, polarity
•
•
Ionization
energy
Periodic Trends
Across period 2/3
Down group 1/17
Atomic/ionic
radii
Gp 1
period 2
period 3
Ionization energy
Atomic radii
Ionic radii
Electronegativity
Melting
point
Electronegativity
Gp 17
Chemical change – diff composition from original substances
- chemical bonds broken/ formed
- new products formed
4. Why IE increases across the period?
Why IE decreases down a group ?
Ionization energy (IE)
1st Ionization energy
Min energy to remove 1 mole e from
1 mole of element in gaseous state
M(g) M+ (g) + e
2nd Ionization energy
Min energy to remove 1 mole e from
1 mole of +1 ion to form +2 ion
M+(g) M2+ (g) + e
Ionization energy
Factors affecting ionization energy
1
2
Distance from nucleus
3
Nuclear charge
electron
+3
+4
+5
+6
Effective Nuclear Charge (ENC)/(Zeff)
• Screening effect/shielding
• Effective nuclear charge (ENC)/(Zeff)
(Zeff) = Nuclear charge (Z) – shielding effect
• Net positive charge felt by valence electrons.
Nuclear charge increase
Distance near to nucleus – IE High
Distance far away nucleus – IE Low
Nuclear charge high (more proton) – IE High
Nuclear charge low (less proton) – IE Low
+6
Inner electron – shield valence e from positive nuclear charge
Distance near
Nuclear charge
Higher electron/electron repulsion
Strong electrostatic forces
attraction bet nucleus and e
Strong electrostatic forces
attraction bet nucleus and e
Easier valence e to leave
IE – High
IE – High
IE – Low
5. IE drop from Be to B and N to O
Ionization Energy- Period 2
Why IE increases across the period 2?
IE increases across period 2
Nuclear charge increase
Strong electrostatic forces
attraction bet nucleus and e
IE – High
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
IE drop from Be to B
1s2 2s2 2p3
1s2 2s2 2p4
IE drop from N to O
Electron in p sublevel of B
– further away from nucleus
2 electrons in same p orbital
- Greater e/e repulsion
Weak electrostatic force attraction
between nucleus and electron
Easier to remove e
IE - Low
IE - Low
period 2
1s2 2s2 2p5
1s2 2s2 2p6
6. IE drop from Mg to AI and P to S
Ionization Energy- Period 3
Why IE increases across the period 3?
IE increases across period 3
Nuclear charge increase
Strong electrostatic forces
attraction bet nucleus and e
IE – High
Na
Mg
AI
Si
P
S
CI
Ar
3p
3s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p1
[Ne] 3s2 3p2
IE drop from Mg to AI
[Ne] 3s2 3p3
[Ne] 3s2 3p4
IE drop from P to S
Electron in p sublevel of AI
– further away from nucleus
2 electrons in same p orbital
- Greater e/e repulsion
Weak electrostatic force attraction
between nucleus and electron
Easier to remove e
IE - Low
IE - Low
Period 3
[Ne] 3s2 3p5
[Ne] 3s2 3p6
7. IE for Period 2 and 3
Ionization Energy- Period 2 and 3
Why IE period 3 lower than 2?
Period 3 – 3 shells/energy level
Period 3
Valence e further from nucleus
High shielding effect – more inner e
Weaker electrostatic forces
attraction bet nucleus and e
IE – Lower
period 2
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
Period 3
Na
Mg
AI
Si
P
S
[Ne] 3s2 3p1
[Ne] 3s2 3p2
[Ne] 3s2 3p3
[Ne] 3s2 3p4
CI
Ar
3rd level
3p
3s
2p
2s
1s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p5
[Ne] 3s2 3p6
8. IE for Ne and Ar
Ionization Energy- Period 2 and 3
Why Ne and Ar have HIGH IE ?
Full electron configuration, 2.8/2.8.8
neon
argon
Most energetically stable structure
Difficult to lose electron
IE – High
period 2
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
Period 3
Na
Mg
AI
Si
P
S
[Ne] 3s2 3p1
[Ne] 3s2 3p2
[Ne] 3s2 3p3
[Ne] 3s2 3p4
CI
Ar
3p
3s
2p
2s
1s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p5
[Ne] 3s2 3p6
9. Atomic Radius
Distance between nucleus and outmost electrons.
Atomic radius
✗
✔
Atom not like a ball – can’t measure its radius directly
Uncertain about position of electron – uncertain of atomic radius
Uncertain abt electron position
How to measure atomic radius?
Half the distance bet nuclei of two closest identical atoms.
Atomic Radius
Covalent Molecule
Noble gas
Monoatomic atoms
Depend on type of bonding – covalent or metallic
Metallic elements
Ionic compounds
½ bond length
½ bond length
½ bond length
Covalent Radius
½ bond length of 2 atom
Van Der Waals radius
½ bond length of nuclei atoms
not bonded together (noble gas)
Click here video on atomic radius
Metallic radius
½ bond length bet nuclei of
neighbouring metal ions
Click here video on atomic radius
Ionic radius
Measure indirectly using
internucleus distance
Click here video on atomic radius
10. Effective Nuclear Charge (ENC)/(Zeff)
• Screening effect/shielding
• Effective nuclear charge (ENC)/(Zeff)
(Zeff) = Nuclear charge (Z) – shielding effect
• Net positive charge felt by valence electrons.
Effective nuclear charge
Effective nuclear charge
magnesium (2.8.2)
net +2
10 inner electron shield 12+ protons
Valence electron feel a net (12-10 = +2)
Calculate Z(eff) and atomic radius for Li
Effective nuclear charge, (Zeff) = +2
1
2
Calculate Z(eff) for Li
Formula
ionization energy
Fcentripetal Fcoulomb
Lithium (2.1)
Z2
IE 1312 2
n
2nd energy level
n=2
Z2
521 1312 2
2
Z eff 1.26
1st IE Li = 521kJ/mol
2 inner electron shield 3+ protons
Calculate atomic radius Li using Z(eff)
R
mv 2 kqZ
2
r
R
2
mh
kqZ
m2 2 R 2
R
h2
R
m 2 kqZ
R 168pm
h
h
p mv
h
v
m
v
h
mR
2nd energy level
n=2
n2
2 2R
R
m = mass electron -9.1 x 10-31
h = plank constant – 6.626 x 10-34
k = coulomb constant – 9.0 x 109
q = charge electron – 1.6 x 10-19
Z = effective nuclear charge - +1.26
Valence electron felt a net (3-2) = +1
Z(eff) = +1.26 NOT +1
(calculation shown above)
Click here video ENC Li
Click here video calculating radius Li
11. Atomic Radius (Covalent radius)
Atomic Radius- Period 2/3
Why atomic radius decrease across period 2/3
Atomic radius decrease across period 2/3
Effective Nuclear charge increase
Strong electrostatic forces
attraction bet nucleus and e
Size decrease
Gp 17
Li
+3
Be
+4
C
+6
N
+7
F
+9
O
+8
Effective Nuclear charge increase
period 2
Na
+11
period 3
B
+5
Mg
+12
AI
+13
Si
+14
P
+15
S
+16
CI
+17
Effective Nuclear charge increase
Why atomic radius increase down Gp 17?
Screening/shielding effect increase
Inner shell electrons
electron electron repulsion increase
Number shell increase
Valence e further away from nucleus
Atomic radius High
12. Positive Ions (+)
Atomic and Ionic Radius- Period 2/3
Ionic radii Positive ion (+) smaller
Negative Ions (-)
Ionic radii Negative ion (-) bigger
Decrease in number of shells – loss of electron
Increase in number of shells – gain of electron
Less electron electron repulsion
Increase electron electron repulsion
Size decrease
Size increase
Comparison bet atomic/ionic radii
Comparison bet atomic/ionic radii
Ionic radii
Ionic radii
Atomic radii
Atomic radii
Na
Mg
AI
2.8.1
2.8.2
2.8.3
Na+
2.8
Mg2+
2.8
AI3+
2.8
Atomic radii
- 3 shells
Ionic radii
- 2 shells
S
2.8.6
S2-
2.8.8
Atomic radii
CI
2.8.7
CI-
2.8.8
- 3 shells
Ionic radii
- 2 shells
13. Electronegativity
Electronegativity (EN)
Tendency of atom to attract/pull shared/bonding electron to itself
EN value higher – pull/attract electron higher (EN value from 0.7 – 4)
•
•
Shared electron cloud closer to O
•
•
EN highest
EN lowest
•
•
Electronegativity
EN increase up a Group
EN increase across a Period
Size
Factors affecting EN value
Size of atom/distance – small size/distance – stronger attraction for electron
Nuclear charge – higher nuclear charge – stronger attraction for electron
Gp 17
EN decrease down gp 17
F
Size increase
Nuclear charge
CI
Attraction electron decrease
EN increase across period 2
Li
+3
EN lower
Be
+4
B
+5
C
+6
N
+7
O
+8
Br
F
+9
Period 2
I
EN increase across period 2
Nuclear charge increase
Strong attraction for electron
EN increase
14. •
•
Melting point across Period 2/3
Melting point down Gp 1/17
Melting Point
•
•
Temp when solid turn to liquid (temp remain constant)
Energy absorb to overcome forces attraction bet molecule
Period 2/3
Melting Point
Gp 1
Gp 17
Factors affecting melting point
Type of bonding/forces
Structure
Metallic/Non Metallic
structure
Covalent
structure
Simple molecular
structure
Ionic
structure
Metallic Bonding
Melting point across Period 2 and 3
Giant molecular
structure
period 2
C
period 3
B
Si
Be
Mg
Li
Na
N O F Ne
AI
P S
Covalent Bonding
CI
Ionic Bonding
15. Melting point for metallic/non metallic
Melting point across Period 2
Melting Point
C
period 2
B
Be
Li
N O F Ne
Li
Be
B
C
N
O
F
Ne
m/p
(/C)
180
1280
2300
3730
-210
-218
-220
-249
structure
metallic
metallic
Giant
covalent
Giant
covalent
Simple
molecular
Simple
molecular
Simple
molecular
metallic
metallic
Giant
covalent
Giant
covalent
Simple
covalent
Simple
covalent
Simple
covalent
Across period 2
m/p increase from Li – C
m/p drop from N – Ne
Metallic – non metallic
Mono
atomic
bonding
•
•
•
Simple
covalent
Metallic bonding
Giant covalent
Simple covalent
Van der waals forces bet molecules
Strong attraction bet
nucleus with sea of electrons
High m/p
Macromolecular structure with
strong covalent bonds
Highest m/p
Simple molecular weak Van Der Waals
forces attraction bet molecules
Low m/p
16. Melting point for metallic/non metallic
Melting point across Period 3
Melting Point
Period 3
Si
Mg AI
Na
Na
Mg
P S
AI
CI Ar
Si
P
S
CI
Ar
m/p
(/C)
98
650
660
1423
44
120
-101
-189
structure
metallic
metallic
metallic
Giant
covalent
Simple
molecular
Simple
molecular
Simple
molecular
metallic
metallic
metallic
Giant
covalent
Simple
covalent
Simple
covalent
Simple
covalent
Across period 3
m/p increase from Na – Si
m/p drop from P – Ar
Metallic – non metallic
Mono
atomic
bonding
•
•
•
Simple
covalent
Metallic bonding
Giant covalent
Simple covalent
Van der waals forces between molecules
Strong attraction bet nucleus
with sea of electrons
High m/p
Macromolecular structure
with strong covalent bonds
Highest m/p
Simple molecular weak Van Der Waals
forces attraction bet molecules
Low m/p
17. Atomic Radius- Group 1 and 17
Ionization Energy – Group 1 and 17
Atomic Radius
Atomic Radius
Atomic Radius
Gp 1
shell
Melting point – Group 1 and 17
Atomic Radius
Ionization Energy
Gp 17
shell
Melting point
Gp 1
Gp 17
Gp 1
Gp 17
Li
F
Li
2.1
F
2.7
Li
F
Na
2.8.1
CI
2.8.7
Na
CI
Na
CI
K
2.8.8.1
2.8.18.7
K
Br
K
Br
Rb
I
Rb
2.8.8.18.1
Br
2.8.18.18.7
I
Why atomic radius increase ?
Number shell increase
Valence e further away from nucleus
Atomic radius High
Rb
I
IE decrease down group
Number shell/energy level increase
Valence e further away from nucleus
Weak forces attraction bet nucleus and e
IE – Low
m/p down Gp 1
Size increase
Attraction bet nucleus and
sea electrons decrease
Metallic bonding
Melting point
m/p increase Gp 17
Size increase
VDF increase
IMF attraction bet
molecules increase
Melting point