Understanding Atomic Structure and Subatomic Particles

Atomic Structure
L/O – Deduce the structure of different elements
 
 
Last week
: 
State
 how you would separate a mixture of a liquid and an
insoluble solid
Last term
: 
Identify 
the type of wave found in water
Last year
: 
Calculate
 the actual size of the section of the onion cells
Key Words
Proton
Neutron
Election
Nucleus
Shell
 
 
 
 
 
 
Resilience: Use various rules to determine atomic mass and structure
 
 
How to Read the periodic table
 
This is Beryllium
 
It’s atomic mass is 9 (this biggest number 
and
atomic number is 4 (the smallest number).
To draw out the atom like below these numbers
are Key
To know how many protons and electrons there
are you look for the atomic number which in
this case is 4. Picture below shows this.
Then to work how many neutrons you the
atomic number away from the atomic mass
which is 9-4= 5 so you now then have 5
neutrons
So the answer would be
Protons:4
Electrons:4
Neutrons:5
 
Atoms are made up of:
Protons – found in the nucleus
Neutrons – found in the nucleus
Electrons – found in shells around the outside of the atom
 
An atom is made up of 3 types of 
subatomic particle
:
Protons
 and 
neutrons
 are found in the 
nucleus
Electrons
 are found around the nucleus in 
electron shells
 
Atomic number = number of protons
Number of protons = number of electrons
Atomic mass = number of protons + number of neutrons
Bronze
:
1.
Deduce 
the number of subatomic particles in 
carbon
, 
lead
,
mercury
 and 
radium.
2.
Explain
 why all of these elements have 
no overall charge
.
Gold:
1.
Produce
 a set of instructions for somebody to calculate the
number of 
protons
, 
neutrons
 and 
electrons
 in an atom using the
periodic table.
2.
Justify
 why a cathode ray tube was able to separate out the
subatomic particles of an atom.
3.
Explain
 why the electron was deflected further than the proton
Silver:
1.
Explain
 why a 
mercury atom
 does not have an overall charge.
Justify whether this is true for all atoms.
2.
Explain
 the difference between the 
atomic number
 and 
mass
number
 for an element.
 
Progress Questions
 
1.
Magnesium contains 12 electrons. It has an electron
configuration of:
a)
6.6
b)
8.4
c)
2.8.2
 
2.
Use the electron configuration of magnesium to identify
which
 group
 and 
period 
of the periodic table it is found
in.
 
3.
Explain what is meant by an 
isotope
.
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Delve into the world of atomic structure and subatomic particles to reveal the inner workings of elements. Discover how to determine atomic mass, identify protons, neutrons, and electrons, and interpret the periodic table. Explore the key concepts of isotopes, electron configurations, and the characteristics of various elements. Enhance your knowledge of chemistry with a focus on the fundamental components of matter.


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  1. Resilience: Use various rules to determine atomic mass and structure Atomic Structure L/O Deduce the structure of different elements Last week: State how you would separate a mixture of a liquid and an insoluble solid Last term: Identify the type of wave found in water Last year: Calculate the actual size of the section of the onion cells Key Words Proton Neutron Election Nucleus Shell

  2. How to Read the periodic table This is Beryllium It s atomic mass is 9 (this biggest number and atomic number is 4 (the smallest number). To draw out the atom like below these numbers are Key To know how many protons and electrons there are you look for the atomic number which in this case is 4. Picture below shows this. Then to work how many neutrons you the atomic number away from the atomic mass which is 9-4= 5 so you now then have 5 neutrons So the answer would be Protons:4 Electrons:4 Neutrons:5

  3. Atoms are made up of: Protons found in the nucleus Neutrons found in the nucleus Electrons found in shells around the outside of the atom

  4. An atom is made up of 3 types of subatomic particle: Protons and neutrons are found in the nucleus Electrons are found around the nucleus in electron shells Atomic number = number of protons Number of protons = number of electrons Atomic mass = number of protons + number of neutrons

  5. Bronze: 1. Deduce the number of subatomic particles in carbon, lead, mercury and radium. 2. Explain why all of these elements have no overall charge. Silver: 1. Explain why a mercury atom does not have an overall charge. Justify whether this is true for all atoms. 2. Explain the difference between the atomic number and mass number for an element. Gold: 1. Produce a set of instructions for somebody to calculate the number of protons, neutrons and electrons in an atom using the periodic table. 2. Justify why a cathode ray tube was able to separate out the subatomic particles of an atom. 3. Explain why the electron was deflected further than the proton

  6. Progress Questions 1. Magnesium contains 12 electrons. It has an electron configuration of: a) 6.6 b) 8.4 c) 2.8.2 2. Use the electron configuration of magnesium to identify which group and period of the periodic table it is found in. 3. Explain what is meant by an isotope.

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