2023 IB Chemistry guide - CHEMSWOT.COM

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2023 IB Chemistry guide - CHEMSWOT.COM

2023 IB Chemistry guide:Are you an IB Chemistry teacher? The 2023 IB DP Chemistry guide for the first assessment in May 2025

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Teaching IB Chemistry in 2023? Get a head start for the first assessment in May 2025 with this guide to the 2023 IB DP Chemistry program. Learn about curriculum structure and content, assessment requirements, and helpful tips to help you prepare all your students for success.

2023 IB Chemistry guide

Page 1 / 89 Are you an IB Chemistry teacher? If so, you'll be happy to know that the 2023 IB DP Chemistry guide for the first assessment in May 2025 is available for download on My IB . It's important for all IB Chemistry teachers to familiarize themselves with the guide, so make sure to take some time to go through it. The guide covers a lot of information about the IB program in general, which might not be new to experienced teachers but is still important to go over. The real chemistry content starts on page 21 with the aims and objectives and continues through page 65 with the syllabus. The rest of the guide explains how the syllabus is assessed and includes important information about command terms.

 Want to know to summarise a set of new assessments in 2025.

Need help understanding the new 2023 IB DP Chemistry guide? This guide provides a comprehensive overview of what you need to know from the syllabus, to the paper topics and more.

Preparing for the IB DP Chemistry examination in 2023? This guide offers a comprehensive breakdown of the syllabus, how to approach each topic, and useful tips and strategies to help you make the most out of your exam preparation.

Understand the syllabus and assessment objectives for every topic.

It is essential that you understand the syllabus and assessment objectives for each topic in 2023 IB DP Chemistry so that you can efficiently plan your study time. The syllabus outlines the topics that need to be covered within each section, providing helpful guidance about which areas you should focus on. Additionally, it provides an overview of the key terms applicable to each subtopic, along with detailed explanation of the assessment objectives that need to be met in order to get a good grade.

Familiarize yourself with the different types of questions in the exams and practice them regularly.

In addition to having a good understanding of the syllabus, you should also be familiar with the different types of questions asked in the IB DP Chemistry exams. This includes multiple choice questions that test factual recall and short response exercises that require more written answers which gives an insight into your depth of knowledge on a topic. It can also help to practice with past papers to get a better idea of what kind of content is expected from you during the assessment. Doing this regularly can help improve your chances in getting a good grade!

Utilize resources like past papers, textbooks and online sources to supplement your learning.

Having access to the right resources is key to succeeding in the IB DP Chemistry course. Use a variety of materials such as textbooks, past papers, and online sources in your studies . Pay special attention to official textbooks prescribed by IB and make sure you understand how concepts and topics are related to one another. Additionally, familiarize yourself with the example questions on past paper exams to get a better idea of what kind of content may appear on your assessment. Doing this regularly will maximize your chances for success!

Learn how to analyze data, apply theories and implement equations where applicable.

A good place to start in mastering the IB DP Chemistry syllabus is to familiarize yourself with data analysis, theories and equations. Understanding these will help you answer questions related to the topics you learn more effectively. Pay special attention to graphs, equations and other visuals which are often used as examples in exams. When applying equations, be sure to pay attention to its units so you can accurately calculate answers and make deductions based on scientific evidence. Doing this regularly will help you gain confidence in problem-solving related activities!

Identify key topics that are most likely to feature in the exam and focus on them during your preparation process.

During your preparation for the IB DP Chemistry exam, it's important to identify what topics among the syllabus are most likely to be included. Many of these topics may have been covered in your school studies and textbook readings. Common key topics usually include Acids and Bases, Vapour Pressure, Lattice Energies and Kinetics. Building a solid understanding on these will help you understand other questions related to them more easily during an exam. Additionally, regularly engaging with past papers also helps you be prepared for any surprises when answering questions since they contain questions iunexpected yet under the scope of the syllabus.

Aufbau Rule and filling of electrons in orbitals and sub shells

Aufbau Rule and filling of electrons in orbitals and sub shells

Aufbau rule is not on the name of any scientist as usually happened in sciences. Aufbau means building up.

Electrons are build up in orbitals of different subshells of different energy levels on the basis of energy.

Electrons first fill lower energy level and then move to next higher level.

So electrons start filling from 1s orbital on wards in the following sequence:

1s,2s,2p , 3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s

Simply it can be learned as ssp sps dps dps fdps fdps

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How do you find oxidation number of an atom?

How do you find oxidation number of an atom?

If you want to learn about oxidation numbers and the method to assign the oxidation number, you should read the following points.

1.    The oxidation state of group 1 elements is always +1. 

Li, Na, K, Rb, Cs, Fr have +1 oxidation state in all the compounds.

                  For example: Oxidation state of Na in Na₂O  is +1.

2.    The oxidation state of group 2 elements is always +2. 

Mg, Ca, Ba etc will always have +2 Oxidation state.

For Example: Oxidation number of Mg in MgO is +2.

3.    The free element or a free molecule will always have oxidation state equal to zero.

For example: Fe and O₂ will have oxidation state equal to zero.

4.    Fluorine is the most electronegative element so it always has -1 oxidation state.

5.    Other halogens generally have -1 oxidation state.

For example: Cl has -1 oxidation state in NaCl.

In Interhalogen compounds like IF_7,  Iodine has +7 Oxidation state because 

Fluorine always have -1 oxidation state.

6.    Oxygen generally have -2 oxidation state in all oxides. 

For example: Oxidation state of O in CO₂  is -2.

In peroxides ,oxidation state of O is -1.

For example: Oxidation state of O in H₂O₂( Hydrogen peroxide) is -1.

In superoxides, Oxidation state of O is -1/2. 

For example; oxidation state of O in NaO₂ ( Sodium superoxide) is -1/2.

Exceptionally oxygen has +2 oxidation state in OF₂( Oxygen fluoride) because F 

has -1 oxidation state always.

7.    The oxidation state of all the ions ( simple ions or polyatomic ion) is always equal 

to the charge on them. 

For example: Oxidation states of Aluminium and phosphate ions is equal to the 

charge on them.   Al³⁺and (PO4)^3-  

8.    The sum of all the oxidation states of all atoms in compounds is always zero.

For example: The sum of all Oxidation states in H₂O=0

H=+1 so +1x2 = +2

O= -2  so the sum is +2 -2= 0

9.    The oxidation states of transition elements isto be determined by using above 

rules because they have variable oxidation states.

The Oxidation state of Mn in KMnO₄  is to be calculated.

K= +1 because it is in group 1.

Mn=?

O=-2 x4= -8

+1+Mn -8= 0

Mn = +7

Worksheet:

Determine the following oxidation states.

1.    N in NO₃^-       

2.    S in H₂SO₄

3.    Cr in K₂Cr₂O₇

4.    Fe in Fe₂O₃

5.    Fe in Fe₃O₄

6.    Mn in MnO₂      

7.    S in SO₃^2-      

8.    C in CH₄      

9.    S in HSO₄^-    

10. N in NO₂^-        

IB Diploma chemistry guide 2019-2020

IB Diploma chemistry guide 2019-2020

You can download IB diploma chemistry guide from the above link.

This is for the students of IB diploma from the 2016 first exams on wards till now.

It is highly recommended for IB Diploma chemistry students to regularly go through the chemistry guide so that you are aware about the syllabus content which is coming in your exams. Students and teachers sometimes ignore the guide which lend them in a time wasting exercise. For example, earlier the working and structure of mass spectrometer was in IB diploma syllabus but now it is not in syllabus so if you are still preparing about the structure and working of mass spectrometer, you are wasting your time. Only the % abundance of isotopes is in syllabus now. 
So to avoid this situation, you should go through the chemistry guide.

Noble prize in chemistry- 2019 for lithium ion batteries

2019 Nobel Prize in chemistry is awarded jointly to three scientists Goodenough, Whittingham and Yoshino for the development of Lithium Ion battery which revolutionized the fueling , working and safety  of the gazettes like mobiles , tablets and computers.

 A lithium-ion battery or Li-ion battery is a secondary cell or rechargeable battery in terms of chemistry.

Primary cell or battery: The cell which cannot be reused once the reactants are finished or the reaction is completed.

Secondary cell or battery: The cell which can be recharged and reused by reversing the chemical reactions.  Once the chemical reactions are completed, the chemical reaction is reversed to get back the reactants by giving electricity to it which we call recharging.

What is a Chemical bond? How is Ionic bond formed?

Powerpoint presentation on Ionic bond

What is a Chemical bond? How is Ionic bond formed? 

The force of attraction between two or more bonded atoms is 

called chemical bond.

There are three types of chemical bonds:

Octet or duplet rule:

The atoms try to become stable by acquiring the electronic structure of nearest noble gas. Except Helium all the noble gases have eight electrons in their outer most shell so atoms try to get eight electrons in the outermost shell. This is called Octet rule.

Atoms become stable by : Lose of outermost electrons( Metals become stable by lose of outermost electrons)

      Gain of electrons( Non-Metals become stable by gain of electrons) or 
       Sharing of electrons(Non-Metals become stable by sharing of electrons)

The atoms near to He try to acquire 2 electrons in their outermost shell to become stable. It is called duplet rule.

 Definition:

The electrostatic force of attraction between two or more oppositely charged ions is called ionic bond.

Example: The electrostatic force of attraction between Sodium ions (Na⁺) and chloride ions( Cl^-) forms an ionic bond.

Metals loose valence electrons to become positive ions

( cations) because cations have more protons than electrons. Na atom has 11 p and 11 e but after lose of 1 e it left with 10 e but 11 p so 1 p is extra means 1 positive charge is extra so it becomes Na.⁺

Na         – 1e àNa⁺

2,8,1                  2,8

Non-Metals gain electrons to become negative ions( anions) because anions have less protons than electrons. Cl atom has 17 p and 17 e but after gain of 1 e it has with 18 e but 17 p so 1 p is less means 1 positive charge is less so it becomes Cl^- .

Cl         +1e à Cl^- 

2,8,7                 2,8,8

Name of the ionic compounds

The cation is the first name

The anion is the second name. The anions generally end with ide like chloride, oxide, nitride etc

The compound ions like phosphate, carbonate, nitrate etc end with ate.

Sulphate ion, SO₄^2-

Phosphate ion, PO₄^3-

Hydrogen carbonate or bicarbonate ionHCO₃^-

Ethanoate (acetate ion), CH₃CO₂^-

Hydroxide ion, OH^-

Nitrate, NO₃^-

Carbonate, CO₃^2-

^{Oxalate ion C}₂^O₄^-

Ammonium ion is a positive ion , NH₄⁺ 

^{Write the names of the following compounds}

Na₂O , NaOH, MgO, Mg(OH)₂, H₂O, Li₂O

LiCl , MgCl₂, P₄O₁₀, SO₂, SiO₂, Al₂O₃ , Al₂(SO₄)₃

Physical properties of ionic compounds

1. High Melting and boiling point- large amount of energy is needed to break the strong electrostatic force of attraction between oppositely charged ions.

2. Crystalline in name – They form crystal lattice ( Large 3D network of ions)

3. Brittle- They breaks easily because of disturbance in the arrangement of ions.

4. Good conductor of electricity in aqueous solutions because of free movement of ions but bad conductor in solid state.

5. Soluble in water because the ions are separated and surrounded by water molecules.

Hydrogen ion concentration in a solution and pH scale

pH is the degree of acidity or basicity of a chemical substance in aqueous systems.

In simple terms pH is the power of hydrogen ion or hydronium ion concentration.

It can be calculated by :
pH = - log₁₀[H⁺] or 

pH = - log₁₀[H₃O⁺] 

[ ] square bracket represents the concentration in mol/dm³

Example: If a sample of an acid is found to have[ H⁺]=1X10^-4

Than pH = - log₁₀[1X10^-4]

pH = -[-4 log 10]

pH= 4
If you want to find out [ H⁺] than you can use the following formula: pH = 10^-pH