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Write the electron configuration for these elements…

Write the electron configuration for these elements…. Label each element from their electron configuration. Nitrogen (N) Sulfur (S) Mangenese (Mn). 2. 2. 6. 2. 6. 2. 1s 2s 2p 3s 3p 4s 1s 2s 2p 3s 3p 1s 2s 2p 3s 3p 4s 3d 4p 5s. 2. 2. 6. 2. 5. 10. 1. 2. 2.

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Write the electron configuration for these elements…

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  1. Write the electron configuration for these elements… Label each element from their electron configuration. Nitrogen (N) Sulfur (S) Mangenese (Mn) 2 2 6 2 6 2 1s 2s 2p 3s 3p 4s 1s 2s 2p 3s 3p 1s 2s 2p 3s 3p 4s 3d 4p 5s 2 2 6 2 5 10 1 2 2 6 2 6 2 6

  2. Periodic Trends

  3. Quick Review • The octet rule • atoms tend to lose or gain electrons in order to attain a full valence shell • Because electrons are negatively charged… • an atom becomes positively or negatively charged as it loses or gains an electron, respectively. • Any atom or group of atoms with a net charge (whether positive or negative) is called an ion. • A positively charged ion is a cation • A negatively charged ion is an anion.

  4. Atomic Size (Atomic Radius) distance between an atom's nucleus and its valence electrons. DECREASING INCREASING

  5. Atomic Size (Atomic Radius) distance between an atom's nucleus and its valence electrons. More Stable Sodium Chlorine Increasing energy levels so electrons are farther from nucleus Cesium

  6. Ionization Energy the energy it takes to fully remove an electron from the atom INCREASING DECREASING

  7. Ionization Energy the energy it takes to fully remove an electron from the atom More Stable Sodium Chlorine Not as tightly bound to the nucleus Cesium

  8. Electronegativity the ability of an atom to attract the electrons of another atom when bonded INCREASING DECREASING

  9. Electronegativity the ability of an atom to attract the electrons of another atom when bonded Gain (attract) electrons to reach octect rule Sodium Chlorine More shielding occurring So less attractive forces Cesium

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