Hello Everyone! Today I will be telling you what we’ve been doing in Science since the start of term 3
1. Parts of an Atom
Atoms are the smallest units of matter and are made up of three types of particles: protons, neutrons, and electrons. Protons have a positive charge and, along with neutrons (which are neutral), are packed together in the atom’s center, called the nucleus. Electrons, which have a negative charge, move rapidly around the nucleus in specific energy levels or shells. In our class, using models or diagrams really helped us visualize what is usually invisible to the eye.
2. What Elements Are
Elements are pure substances that can’t be broken down into simpler substances by normal chemical means. Each element is made of only one kind of atom, such as hydrogen, carbon, or oxygen. We explored models and periodic table charts to see how each element is unique.
3. Reading the Periodic Table
The periodic table is like an encyclopedia for elements. Each box on the table tells you the element’s chemical symbol, atomic number (number of protons), and atomic mass (average mass of an atom, considering protons and neutrons). As a class, we practiced identifying key information about elements just by looking at the table.
4. Calculating Protons, Electrons, Neutrons
To find the number of protons, look at the atomic number. In neutral atoms, electrons equal protons. Neutrons are found by subtracting the atomic number from the mass number (atomic mass rounded to the nearest whole number). Doing these calculations in class made us realize how these tiny changes give each element its unique characteristics.
5. Electron Orbits
Electrons orbit the nucleus at different energy levels or shells. The way they fill the shells follows specific rules (the 2-8-8 rule for the first three shells), which we learned to apply to different elements. Using paper models or digital simulations in class brought this concept to life.
6. Electron Configuration
This is a shorthand way to show how electrons are arranged among the shells. For example, carbon’s configuration is 2,4. We enjoyed writing these out for various elements and comparing how similar or different they can be.
7. Ions and Formation
Atoms can gain or lose electrons, becoming ions—charged particles. Losing electrons makes a positive ion, gaining makes a negative ion. We experimented with salt solutions to actually see ion formation in action.
8. Word Equations
A word equation uses words to describe reactants and products of a chemical reaction, like “hydrogen + oxygen → water.” We got experience writing these by describing real lab reactions.
9. Elements, Compounds, Mixtures
Elements contain only one type of atom. Compounds have atoms of different elements that are chemically bonded, while mixtures combine substances physically, not chemically. Lab tests—like separating sand from saltwater—helped us spot the differences.
10. Chemical Formula
A chemical formula uses symbols and numbers to show the atoms in a compound, such as H2O. Writing formulas during experiments helped us link what we saw in the lab with chemical notation.
11. Counting Atoms
By breaking down formulas, we counted the number of each type of atom—like two hydrogens and one oxygen in H2O. Hands-on practice with molecular models made this easier to understand.
12. Balancing Symbol Equations
Balancing equations ensures both sides have the same number of each atom. We learned this by practicing on whiteboards, which was challenging but satisfying when everything balanced!
13. Properties of Metals
Metals are shiny, conduct electricity, are malleable (bendable), ductile (can be drawn into wires), and usually solid at room temperature. Observing and testing different metals in class let us see these traits firsthand.
14. Uses of Metals
We looked at why certain metals are used for specific things (like copper in wires, aluminum in foil), linking their properties to their uses with real-life examples.
15. Alloys
Alloys are mixtures of metals with other elements to improve properties, like making them stronger or more resistant to rust (e.g., stainless steel). We observed what happens to pure metals versus alloys in corrosion experiments.
16. Corrosion Experiment
We studied how metals react with water, air, or acids—like rust forming on iron. Recording changes over time in our logs helped us understand how environmental factors affect metals.
17. Identifying Products
By looking at reactants, we predicted and tested what products would form in a reaction. For example, mixing baking soda and vinegar produced gas (carbon dioxide), which bubbled visibly.
18. Scientific Experiments
We summarized experiment results in tables and wrote blog posts to reflect on what we’d learned, which reinforced our understanding and communication skills.
19. Acids and Bases
Acids taste sour, turn litmus paper red, and release hydrogen ions (H+). Bases taste bitter or feel slippery, turn litmus blue, and release hydroxide ions (OH-). We tested household substances to categorize them as acids or bases.
20. pH Scale
The pH scale (0-14) measures how acidic or basic something is. We used pH paper or digital testers to check the pH of various common liquids.
21. Indicators
Indicators change color depending on acidity or basicity (like litmus or universal indicator). We learned how essential they are for identifying acids and bases.
22. Making Indicators
We made our own natural indicators (like red cabbage juice!) and tested different substances, which was a fun hands-on activity.
23. Scientific Reports
Writing up our experiments in a proper structure helped us communicate our findings clearly, like real scientists.
24. Neutralization Reaction
When acids and bases react, they form water and a salt. We mixed vinegar and baking soda, observing fizzing and recording results.
25. Neutralization Equation
The general equation is acid + base → salt + water. Practicing this with different acids and bases helped us see the pattern.
That is all for today.
Thank You.
