Molecular compounds are formed when two or more different non-metal atoms combine via covalent bonds, sharing electron pairs. Examples include water, which is made of two hydrogen atoms bonded to one oxygen atom. Molecular compounds have properties like being soft and having low melting points. They are named systematically with the first element, the second as an "-ide", and prefixes to indicate atom amounts, like dinitrogen monoxide for N2O.
8th Grade Integrated Science Chapter 8 Lesson 1 on Electrons and Energy Levels. This lesson gives a brief introduction of the periodic table, periods, and groups. There is an introduction to metals, nonmetal, and metalloids. This also introduces electrons, energy levels, and the basic idea of bonding.
Organic compounds are almost 60% of all compounds. because of carbons tendency to form a compound as it has more than1 electron(4electrons) to form covallent compounds. SO a wide range of everything we eat is formed from carbon and hydrogen, which is the second important element to form organic compounds.
It is a powerpoint presentation that discusses about the lesson or topic: Percentage Composition. It also talks about the definition, concepts and examples about the Percentage Composition.
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
8th Grade Integrated Science Chapter 8 Lesson 1 on Electrons and Energy Levels. This lesson gives a brief introduction of the periodic table, periods, and groups. There is an introduction to metals, nonmetal, and metalloids. This also introduces electrons, energy levels, and the basic idea of bonding.
Organic compounds are almost 60% of all compounds. because of carbons tendency to form a compound as it has more than1 electron(4electrons) to form covallent compounds. SO a wide range of everything we eat is formed from carbon and hydrogen, which is the second important element to form organic compounds.
It is a powerpoint presentation that discusses about the lesson or topic: Percentage Composition. It also talks about the definition, concepts and examples about the Percentage Composition.
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
The compounds which are made up of ions are known as ionic compounds.
In an ionic compound, the positively charged ions and negatively charged ions are held together by the strong electrostatic forces of attraction.
The forces which hold the ions together in an ionic compound are known as ionic bonds and electrovalent bonds.
A 2000+ slide PowerPoint presentation from www.sciencepowerpoint.com becomes the roadmap for an amazing learning experience. Complete with homework package, built-in activities with directions, built-in quizzes, unit notes, follow along worksheets, answer keys, video links, review games, rubrics, and much more.
Also included are directions on how create a student version of the unit that is much like the teachers but missing the answer keys, quizzes, PowerPoint review games, hidden box challenges, owl, and surprises meant for the classroom. This is a great resource to distribute to your students and support professionals and will only take you a few minutes to create.
This is a great introductory unit that covers science topics associated with Lab Safety, Magnification, Base Units of the Metric System, Scientific Method, Inferences, and Observation Skills (See list below for more topics covered). This unit includes an interactive and engaging PowerPoint Presentation of 2000 slides with built in class notes (Red Slides), lab activities, project ideas, discussion questions, assessments (Quiz Wiz), and challenge questions with answers.
Text is in large print (32 font) and is placed at the top of each slide so it can seen and read from all angles of a classroom. A shade technique, as well as color coded text helps to increase student focus and allows teacher to control pace of the lessons. Also included is a 10 page assessment / bundled homework that chronologically follows the slideshow for nightly homework and end of the unit assessment, as well as a 9 page modified assessment. 14 pages of class notes with images are also included for students who require modifications, as well as answer keys to both of the assessments for support professionals, teachers, and home school parents. Several video links are provided and a slide within the slideshow cues teacher / parent when the videos are most relevant to play. Video shorts usually range from 2-7 minutes. One PowerPoint review game (125+ slides)is included. Answers to the PowerPoint review game are provided in PowerPoint form so students can self-assess. Lastly, several class games such as guess the hidden picture beneath the boxes, and the find the hidden owl somewhere within the slideshow are provided. Difficulty rating of 5 (Ten is most difficult)
Thank you for time and if you have any questions please feel free to contact me at www.sciencepowerpoint@gmail.com. Best wishes.
Teaching Duration = 4+ Weeks
Sincerely,
Ryan Murphy M.Ed
Science PowerPoints
ELEMENTARY PARTICLES OF MATTER
Matter is made up of discrete particles, the main ones are:-
1. Atoms 2. Ions 3. Molecules - (AIM)
DEFINITION OF ATOMS
An atom is the smallest particle of an element which can take part in a chemical reaction
THE CONSTITUENTS OF ATOMS
Rutherford in 1911 threw more light on the nature of the atom. He demonstrated that atom is made up of sub-particles which are called:
1. Proton 2. Neutron 3. Electron.
He discovered that the protons and neutrons are concentrated in the nucleus of an atom, while the electrons are revolving round the nucleus.
J.J THOMPSON’S MODEL
J.J Thompson described the atom as being made up of a mixture of positive (Protons) and negative (Electrons) charges.
LORD RUTHERFORD’S MODEL
Lord Rutherford described the atom as being made up of Positive (Protons) and Neutral (Neutrons) charges in its centre (nucleus) while the negative charges (electrons) rotates around its orbit.
He used the planetary bodies rotating around the sun to describe the structure of atoms.
CHARACTERISTICS OF PROTON, ELECTRON AND NEUTRON
DALTON’S ATOMIC THEORY
In 1808, John Dalton proposed the Atomic Theory which can be summarised as follows:
All elements are made up of small, indivisible particles called atoms.
Atoms can neither be created nor destroyed.
Atoms of the same elements are alike in every aspect, and differ from atoms of all other elements.
When atoms combine with other atoms, they do so in simple ratios.
All chemical changes result from the combination or the separation of atoms.
The Atomic Theory was partially supported by experimental evidences deduced from the Law of Conservation of Mass, the Law of Definite Proportions, the Law of Multiple Proportions and so on. It could not explain electrolysis and certain other phenomena. As a result of new discoveries, Dalton’s original Atomic Theory has undergone several modifications but the principal aspects as outlined above are still useful in the study of chemistry.
MODIFICATIONS OF DALTON’S ATOMIC THEORY
All Elements Are Made Up Of Small Indivisible Particles Called Atoms: This statement has been proven wrong by Rutherford’s discovery – the atom is built up of three main types of sub-particles: the proton, the electron, the neutron. It is not an indivisible solid piece.
The Atom Can Neither Be Created Nor Destroyed: This statement still holds good for ordinary chemical reactions and is embodied in the basic Law of Conservation of Mass. During a nuclear reaction, such as the fission of Uranium – 235, the nucleus is broken up into smaller units which form simpler atoms while a tremendous amount of heat energy is released. These changes that occur during nuclear fission destroy the atoms of the element involved.
The Atoms Of The Same Elements Are Alike In Every Aspect And Differ From Atoms Of All Other Elements: The discovery of isotopes makes this statement unacceptable. Chlorine, for example has two different atom
2. Molecular Compounds
• A molecule is a combination of
two or more atoms held
together by covalent bonds
• A covalent bond occurs
between the atoms of non-
metals in which the two atoms
share a pair of electrons
3. Molecular Elements
• A molecular element is when
two or more atoms of the same
element are joined by covalent
bonds
• A diatomic molecule is a
molecule that is made from two
atoms e.g.) the element chlorine
is a diatomic molecule (Cl2)
4. Molecular Compounds
• When atoms of two or more
different non-metals combine,
a pure substance known as a
molecular compound is
formed
5. Molecular Compounds
• As with molecular elements,
the atoms in molecular
compounds are joined
together by covalent bonds
• In each bond, the atoms share
a single pair of electrons.
6. Molecular Compounds
• For example, water is a
molecular compound with two
covalent bonds
• Each hydrogen atom shares
one pair of electrons with an
oxygen atom
7. Properties of Molecular
Compounds
• soft
• low melting point
• solutions do not conduct
electricity
8. Naming Molecular
Compounds
For compounds that do not
contain hydrogen:
1. Name the first element
2. Name the second element and
change the ending to “-ide”
3. add prefixes to indicate the
number of each atom
9. Naming Molecular
Compounds
• The prefix “mono” is not used
when there is only one atom
of the first element
• When “mono” is being added
to oxygen, the last “o” is
dropped (e.g. “monoxide” not
“monooxide”)
10. Naming Molecular
Compounds
Example 1: N2O
• Name the first element:
nitrogen
• Name the second element
using “-ide”: oxide
• Add prefixes:
dinitrogen monixide
11. Naming Molecular
Compounds
Example 2: PBr3
• Name the first element:
phosphorous
• Name the second element
using “-ide”: bromide
• Add prefixes:
phosphorous tribromide
12. Naming Molecular
Compounds
• Hydrogen is unique in many
ways, and this is reflected in the
naming systems
• Many compounds containing
hydrogen have been given
simpler names
• For example, dihydrogen
monoxide (H2O) is simply
called “water”