Presentation
ATOMIC STRUCTURE
Form 4 Chemistry
The basic building block of matter
ATOMS
VIDEO
A brief history on the development of the atom and all its particles
Sub Atomic Particles
Protons
Neutrons
Electrons
Found outside the nucleus orbiting the nucleus in shells. Have a relative charge of -1 Have a relative mass of 1/1836 or 1/1840 or sometimes it is written as 0
Found inside the nucleus Have a relative charge of +1 Have a relative mass of 1.
Found inside the nucleus Have a relative charge of 0 Have a relative mass of 1
1. Summary
Sub atomic particles
Atomic number is the number of protons in the nucleus of one atom of an element.
Nuclear notation is a way of showing both the mass number and atomic number of an atom of an element.
Mass number is the total number of protons and neutrons in the nucleus of one atom of an element.
CSEC Chemistsry by Anne Tindale page 18
VIDEO
Quick quiz
1. What element does the symbol represent?2. How many protons are found in one atom of this element? 3. How many electrons are found in one atom of this element? 4. How many neutrons are found in one atom of this element?
Electronic Structure/Electronic Configuration
The arrangement of electrons in energy levels or shells around the nucleus
Key points in drawing electronic configurations
When drawing electronic configurations1. Draw in your nucleus separately from your energy shells. Put the atom's symbol in the nucleus and write in the no of protons and neutrons as p=.. and n=.. 2. Start putting electrons in the lowest energy level first. 3. Add your electrons singly at first before you pair them up. Place them at the four cardinal points when drawing them singly 4. The maximum on the 1st shell is 2 and the other shells is 8 5. When WRITING electronic configurations, the order of filling shells is the same as when drawing and commas are placed between the numbers.
VIDEO
How to draw and write electron structure/configurations
So what exactly are ions?
Once the number of protons and electrons are NO LONGER EQUAL in at atom, the species is now called an ION. Ions are formed when atoms lose or gain valence electrons. Electrons are lost or gained when atoms bond with each other to get a full shell to become stable. In Chemistry, all things tend towards stability. (Valence electrons=electrons in the outer shell of the atom)
VIDEO
Let's practise.
Now that we understand how ions are formed, let's practise with an example.1. The atomic number of Na=11. What does that mean? Write down the electronic configuration of the Na atom 2. When sodium reacts, it forms a positive ion. What does that mean, does it lose or gain electrons? 3. How many electron(s) does sodium lose? Why does it lose only this amount? After it forms an ion, write down the number of protons and electrons in the sodium ion. Compare this with the sodium atom in question 1 above. Write or draw the electronic configuration of the sodium ion.
Practice time: Attempt the following questions below
Click here to see the answers
Let's talk isotopes
These are atoms of the SAME ELEMENT with the same number of protons but a different number of neutrons so the mass number is different.
Isotopes
So if an element contains many atoms and some of these atoms may have different mass numbers from each other, can we work out an average mass number for each element?
Question time
Calculating average mass numbers/relative atomic masses
1. Carbon has 3 naturally occuring isotopes with the following relative abundances 98.89% carbon-12, 1.10% carbon-13 and 0.01% carbon-14. Calculate its relative atomic mass (average mass number) to 3 d.p.2. Neon also has 3 isotopes of the following composition 90.48% neon-20, 0.27% neon-21 and 9.25% neon-22. Calculate its average mass to 3dp. Once you have attempted both questions click to see the correct answer
VIDEO 1
What's so special about isotopes anyway?Click here to see more. Refer to page 45-47 of CSEC Chemistry by Naresh Birju or page 21 of the Concise Chemistry by Anne Tindale
VIDEO
This video focuses on the disaster that happened at a nuclear power plant involving of a particular radioactive isotope Uranium 235
Thanks for viewing
Remember that an ion has a different number of electrons from the protons because the electrons AND ONLY THE ELECTRONS are lost or gained during chemical bonding
A positively charged ion or cation will have less electrons than protons. So for Mg2+ the atomic number =12 It has 12 protons, but with a charge on the ion of 2+ , it means that we have 2 MORE PROTONS THAN ELECTRONS [or 2 less electrons than protons as 2 electrons were lost]. The number of electrons=10
A negatively charged ion or anion will have more electrons than protons. So for Cl- with a charge on the ion of 1-, it means that we have ONE MORE ELECTRON THAN PROTONS. The atomic number will first be found by subtracting the mass number 35 and the number of neutrons 18, 35-18=17. There are 17 protons but because it is Cl- as explained above, we will have 18 electrons.
Atomic structure
Janine Bailey
Created on October 13, 2020
Start designing with a free template
Discover more than 1500 professional designs like these:
View
Animated Chalkboard Presentation
View
Genial Storytale Presentation
View
Blackboard Presentation
View
Psychedelic Presentation
View
Chalkboard Presentation
View
Witchcraft Presentation
View
Sketchbook Presentation
Explore all templates
Transcript
Presentation
ATOMIC STRUCTURE
Form 4 Chemistry
The basic building block of matter
ATOMS
VIDEO
A brief history on the development of the atom and all its particles
Sub Atomic Particles
Protons
Neutrons
Electrons
Found outside the nucleus orbiting the nucleus in shells. Have a relative charge of -1 Have a relative mass of 1/1836 or 1/1840 or sometimes it is written as 0
Found inside the nucleus Have a relative charge of +1 Have a relative mass of 1.
Found inside the nucleus Have a relative charge of 0 Have a relative mass of 1
1. Summary
Sub atomic particles
Atomic number is the number of protons in the nucleus of one atom of an element.
Nuclear notation is a way of showing both the mass number and atomic number of an atom of an element.
Mass number is the total number of protons and neutrons in the nucleus of one atom of an element.
CSEC Chemistsry by Anne Tindale page 18
VIDEO
Quick quiz
1. What element does the symbol represent?2. How many protons are found in one atom of this element? 3. How many electrons are found in one atom of this element? 4. How many neutrons are found in one atom of this element?
Electronic Structure/Electronic Configuration
The arrangement of electrons in energy levels or shells around the nucleus
Key points in drawing electronic configurations
When drawing electronic configurations1. Draw in your nucleus separately from your energy shells. Put the atom's symbol in the nucleus and write in the no of protons and neutrons as p=.. and n=.. 2. Start putting electrons in the lowest energy level first. 3. Add your electrons singly at first before you pair them up. Place them at the four cardinal points when drawing them singly 4. The maximum on the 1st shell is 2 and the other shells is 8 5. When WRITING electronic configurations, the order of filling shells is the same as when drawing and commas are placed between the numbers.
VIDEO
How to draw and write electron structure/configurations
So what exactly are ions?
Once the number of protons and electrons are NO LONGER EQUAL in at atom, the species is now called an ION. Ions are formed when atoms lose or gain valence electrons. Electrons are lost or gained when atoms bond with each other to get a full shell to become stable. In Chemistry, all things tend towards stability. (Valence electrons=electrons in the outer shell of the atom)
VIDEO
Let's practise.
Now that we understand how ions are formed, let's practise with an example.1. The atomic number of Na=11. What does that mean? Write down the electronic configuration of the Na atom 2. When sodium reacts, it forms a positive ion. What does that mean, does it lose or gain electrons? 3. How many electron(s) does sodium lose? Why does it lose only this amount? After it forms an ion, write down the number of protons and electrons in the sodium ion. Compare this with the sodium atom in question 1 above. Write or draw the electronic configuration of the sodium ion.
Practice time: Attempt the following questions below
Click here to see the answers
Let's talk isotopes
These are atoms of the SAME ELEMENT with the same number of protons but a different number of neutrons so the mass number is different.
Isotopes
So if an element contains many atoms and some of these atoms may have different mass numbers from each other, can we work out an average mass number for each element?
Question time
Calculating average mass numbers/relative atomic masses
1. Carbon has 3 naturally occuring isotopes with the following relative abundances 98.89% carbon-12, 1.10% carbon-13 and 0.01% carbon-14. Calculate its relative atomic mass (average mass number) to 3 d.p.2. Neon also has 3 isotopes of the following composition 90.48% neon-20, 0.27% neon-21 and 9.25% neon-22. Calculate its average mass to 3dp. Once you have attempted both questions click to see the correct answer
VIDEO 1
What's so special about isotopes anyway?Click here to see more. Refer to page 45-47 of CSEC Chemistry by Naresh Birju or page 21 of the Concise Chemistry by Anne Tindale
VIDEO
This video focuses on the disaster that happened at a nuclear power plant involving of a particular radioactive isotope Uranium 235
Thanks for viewing
Remember that an ion has a different number of electrons from the protons because the electrons AND ONLY THE ELECTRONS are lost or gained during chemical bonding A positively charged ion or cation will have less electrons than protons. So for Mg2+ the atomic number =12 It has 12 protons, but with a charge on the ion of 2+ , it means that we have 2 MORE PROTONS THAN ELECTRONS [or 2 less electrons than protons as 2 electrons were lost]. The number of electrons=10 A negatively charged ion or anion will have more electrons than protons. So for Cl- with a charge on the ion of 1-, it means that we have ONE MORE ELECTRON THAN PROTONS. The atomic number will first be found by subtracting the mass number 35 and the number of neutrons 18, 35-18=17. There are 17 protons but because it is Cl- as explained above, we will have 18 electrons.