electronconfiguration-250218025058-c21bab83.pptx

Electron configuration describes how electrons are arranged in an atom’s orbitals—like a seating chart for electrons around the nucleus. It follows a specific order based on energy levels and sublevels, helping us understand an element’s chemical behavior, reactivity, and placement in the periodic table.

1. Electron configuration ALVIN G. JUANINO

2. In an atom, electrons and the nucleus interact to make the most stable arrangement possible. The way in which electrons are distributed in the different orbitals around the nucleus of an atom is called the electron configuration .

3. No atom actually has more than 32 electrons in any of its principal levels. Orbitals have specific energy values. They have particular shapes and direction in space

4. Parts of an electron configuration: • Principal Energy Level – a number (1, 2, 3, 4, 5, 6, 7) • Sublevel – a letter (s, p, d, f) • Number of electrons – a superscript number (2, 6, 10, 14) Principal Energy Level – a number (1, 2, 3, 4, 5, 6, 7) Sublevel – a letter (s, p, d, f) Number of electrons – a superscript number (2, 6, 10, 14)

5. Example:

6. How to write the electron configuration In writing the electron configuration, when the electrons fill the orbitals, they occupy the lowest energy orbitals that are available. And keep in mind that each orbital can accommodate a maximum of two electrons. Just follow the arrow in the chart, write the principal energy level, sublevel, and the number of electrons. The electron configuration depends on the atomic number of the elements.

7. Basically, the above information can be summed up into 3 rules that define how electrons can be arranged in an atom’s orbital. Aufbau Principle – electrons fill the orbitals one at a time, starting with the lowest energy orbital then proceeding to the one with higher energy. Hund’s Rule – single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals. Pauli Exclusion Principle – states that only two electrons occupy an orbital, and they must have opposite spins.

8. Activity GIVE THE ELECTRON CONFIGURATION OF THE FF. ELEMENTS CARBON - 6 CALCIUM - 20 CHLORINE - 17 ALUMINIUM - 13 POTASSIUM - 19

9. EXPERIMENT TIME!!! PREPARE ONE WHOLE MELTING POINT COMPARISON Materials: Sodium Chloride (table salt) Napthalene or wax C. Fire source D. Thermometer PROcEDURE: I. Heat each compound separately II.. Record the temperature at which each begins to melt

10. EXPERIMENT TIME!!! PREPARE ONE WHOLE Solubility comparison Materials: Sodium Chloride (table salt), sugar, iodine, napthalene C. water, acetone, ethanol D. Small beaker PROcEDURE: Add small amount of each compound to 20 ml water, acetone and ethanol Stir and observe solubility

11. EXPERIMENT TIME!!! PREPARE ONE WHOLE HARdNESS TEST Materials: Sodium Chloride (table salt), sugar B. MORTAR and Pestle PROcEDURE: Crush each compound 25 times

12. EXPERIMENT TIME!!! PREPARE ONE WHOLE Guide questions: MELTING POINT TEST Which of the materials are the covalent or ionic? What material melt in higher temperature? Why do you think so? Solubility test Which of the used materials are covalent or ionic? What material/s dissolved in water, acetone or ethanol? Why they dissolve differently ? HARDNESS TEST 1. after, trying of crushing the compounds what do you think is the harder? Why do you think so?