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How Electrons Determine Chemical Behavior. bonding. patterns of the periodic table. Imagine cars driving into a parking lot for a sports event or concert. For maximum efficiency, parking lot workers direct them to fill each row before a new row is started.
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patterns of the periodic table Imagine cars driving into a parking lot for a sports event or concert. For maximum efficiency, parking lot workers direct them to fill each row before a new row is started. That’s how electrons fill energy levels.
Filling Order Scientists have deduced there is a specific order in which electrons fill the energy levels. Energy maximum levelcapacity s can hold 2 electrons p can hold 6 electrons d can hold 18 electrons f can hold 32 electrons correspondsto period Using these two charts and your periodic table, you can work out the electron configuration of any element.
Contains s subshell Contains s and p subshells nucleus Contains s, p and d subshells Contains s, p, d and f subshells Energy levels -- atomic model Electrons fill the innermost (s) shell first. Then they fill the next innermost shell (p) and so on…
The pattern of filling can also be charted along the periods of the periodic table. Filling order Phosphorus Atomic #15 1s22s22p63s23p3 Five electrons in the outer (3) energy level. It takes less energy to gain 3 than to lose 5. Phosphorus will be an electron receiver. Use this chart and your periodic table to write the electron configurations for: calcium (Ca), molybdenum (Mo), silver (Ag), sodium (Na), and bromine (Br)
how do electrons determine bonding? OCTET RULE: Atoms tend to gain, lose or share electrons so as to have a full outer electron shell.
how do electrons determine bonding? example: Atoms tend to gain, lose or share electrons so as to have a full outer electron shell. 4s1 3s23p5 19 protons18 electrons 17 protons18 electrons has 1valenceelectron needs 1 valenceelectron
how do electrons determine bonding? example: Atoms tend to gain, lose or share electrons so as to have a full outer electron shell. EXAMPLE: Hydrogen has one valence electron. It will offer this electron for bonding to reach its most stable state. Oxygen has six valence electrons. To reach its most stable state it must gain 2. (Too much energy to lose 6). Oxygen’s electronegativity is stronger than Hydrogen’s. It will attract 2 Hydrogen atoms to fill each of its spaces.
