Aim: What is the internal structure of an atom? DO
Description: Aim: What is the internal structure of an atom? DO NOW: Prepare for quiz. Need pen or pencil, and reference tables. Atomic Structure A) Nucleus Proton Neutron B) Electron Cloud 3) Electron The Three Fundamental Subatomic Particles Nucleus
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slide1. Aim: What is the internal structure of an atom? DO NOW: Prepare for quiz. Need pen or pencil, and reference tables.<br>
slide2. Atomic Structure A) Nucleus
Proton
Neutron
B) Electron Cloud
3) Electron<br>
slide3. The Three Fundamental Subatomic Particles<br>
slide4. Nucleus (Protons and Neutrons) 1) Contains most of the mass of the atom; very dense
2) Has a positive charge (nuclear charge)
Charge from protons
Neutrons have no charge<br>
slide5. Atomic Number and Atomic Mass Atomic # = # of protons only
Atomic mass or mass # is both mass of neutron and proton<br>
slide6. Atomic Number and Atomic Mass on Periodic Table<br>
slide7. Neutral Atom If an atom is neutrally charged, what must be true about the number of protons and the number of electron?
In a neutral atom, the # of electrons = # of protons
The protons “hold the electrons in the atoms”
The number of protons (atomic #) determines the element you have<br>
slide8. Sample Problems 1. Lithium has 3 protons and 4 neutron. What is the mass number?
Mass # = # of protons + # of neutrons
Mass # = 3 + 4
Mass # = 7
2. An atom has a mass number of 9 and has 5 neutrons. How many protons does it have?
Mass # = # of protons + # of neutrons
9 = # of protons + 5
# of protons = 4<br>
slide9. Electronic Structure Electrons are found in orbitals outside the nucleus
An orbital is defined as the most probable location of an electron
Electrons are arranged in different shells around the nucleus; each can only hold a certain number of electrons.
The innermost shell is filled first.
Electrons closer to the nucleus have less energy than electrons further away from the nucleus.<br>
slide10. Electronic Structure Cont. Green = proton
Blue= neutron
Red= electron
Which element is this? How can we tell?
How many electrons are in the first shell? Second shell?<br>
slide11. Electronic Structure Cont.<br>
slide12. Electron Shells<br>
slide13. Sample Problem What is the mass number of Magnesium?
Explain from this diagram why the aluminum atom is neutral.<br>
slide14. Symbol for Carbon Carbon-12 or 12C:
It tells us that a carbon atom has:
Six protons (because its proton number, at the bottom, is 6)
Six electrons (because the number of protons and electrons in an atom is the same)<br>
slide15. Isotope of Hydrogen What stays the same in each isotope of hydrogen?
What changes?<br>
slide16. Isotopes of Hydrogen and Chlorine<br>
slide17. What are Isotopes? Atoms of an element that:
Have the same number of protons and electrons
Have different number of neutrons, and therefore have different atomic masses<br>
slide18. Discussion Why are isotopes of an element still of the same element even though they have different number of neutrons between them?<br>
slide2. Atomic Structure A) Nucleus
Proton
Neutron
B) Electron Cloud
3) Electron<br>
slide3. The Three Fundamental Subatomic Particles<br>
slide4. Nucleus (Protons and Neutrons) 1) Contains most of the mass of the atom; very dense
2) Has a positive charge (nuclear charge)
Charge from protons
Neutrons have no charge<br>
slide5. Atomic Number and Atomic Mass Atomic # = # of protons only
Atomic mass or mass # is both mass of neutron and proton<br>
slide6. Atomic Number and Atomic Mass on Periodic Table<br>
slide7. Neutral Atom If an atom is neutrally charged, what must be true about the number of protons and the number of electron?
In a neutral atom, the # of electrons = # of protons
The protons “hold the electrons in the atoms”
The number of protons (atomic #) determines the element you have<br>
slide8. Sample Problems 1. Lithium has 3 protons and 4 neutron. What is the mass number?
Mass # = # of protons + # of neutrons
Mass # = 3 + 4
Mass # = 7
2. An atom has a mass number of 9 and has 5 neutrons. How many protons does it have?
Mass # = # of protons + # of neutrons
9 = # of protons + 5
# of protons = 4<br>
slide9. Electronic Structure Electrons are found in orbitals outside the nucleus
An orbital is defined as the most probable location of an electron
Electrons are arranged in different shells around the nucleus; each can only hold a certain number of electrons.
The innermost shell is filled first.
Electrons closer to the nucleus have less energy than electrons further away from the nucleus.<br>
slide10. Electronic Structure Cont. Green = proton
Blue= neutron
Red= electron
Which element is this? How can we tell?
How many electrons are in the first shell? Second shell?<br>
slide11. Electronic Structure Cont.<br>
slide12. Electron Shells<br>
slide13. Sample Problem What is the mass number of Magnesium?
Explain from this diagram why the aluminum atom is neutral.<br>
slide14. Symbol for Carbon Carbon-12 or 12C:
It tells us that a carbon atom has:
Six protons (because its proton number, at the bottom, is 6)
Six electrons (because the number of protons and electrons in an atom is the same)<br>
slide15. Isotope of Hydrogen What stays the same in each isotope of hydrogen?
What changes?<br>
slide16. Isotopes of Hydrogen and Chlorine<br>
slide17. What are Isotopes? Atoms of an element that:
Have the same number of protons and electrons
Have different number of neutrons, and therefore have different atomic masses<br>
slide18. Discussion Why are isotopes of an element still of the same element even though they have different number of neutrons between them?<br>