際際滷

際際滷Share a Scribd company logo

ionic bond

Download as PPT, PDF
M
Manish Parker

1) Atoms are made up of electrons, protons and neutrons. Electrons occupy electron shells and determine how an atom bonds with other atoms. 2) Ionic bonds form when a metal transfers electrons to a nonmetal, giving them opposing charges. For example, sodium (Na) transfers an electron to chlorine (Cl), forming sodium ion (Na+) and chloride ion (Cl-). 3) Covalent bonds form when atoms share electrons to fill their outer electron shells in a stable configuration.

1 of 27
Downloaded 43 times
ionic bond
Atom the smallest unit of matter indivisible Helium atom
electron shells a) Atomic number = number of Electrons b) Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells. a) Electron shells determine how an atom behaves when it encounters other atoms
Electrons are placed in shells according to rules: 1) The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons.
Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to Gain 4 electrons Gain 3 electrons Gain 2 electrons
Why are electrons important? 1) Elements have different electron configurations different electron configurations mean different levels of bonding
ionic bond
Electron Dot Structures Symbols of atoms with dots to represent the valence- shell electrons 1 2 13 14 15 16 17 18 H He: Li Be B C N O : F :Ne : Na Mg Al Si P S :Cl :Ar :
Chemical bonds: an attempt to fill electron shells 1. Ionic bonds 2. Covalent bonds 3. Metallic bonds
IONIC BOND bond formed between two ions by the transfer of electrons
Formation of Ions from Metals Ionic compounds result when metals react with nonmetals Metals lose electrons to match the number of valence electrons of their nearest noble gas Positive ions form when the number of electrons are less than the number of protons Group 1 metals 錚р ion 1+ Group 2 metals 錚р ion 2+ Group 13 metals 錚р ion 3+
Formation of Sodium Ion Sodium atom Sodium ion Na e 錚эр Na + 2-8-1 2-8 ( = Ne) 11 p+ 11 p+ 11 e- 10 e- 0 1+
Formation of Magnesium Ion Magnesium atom Magnesium ion Mg 2e 錚р Mg2+ 2-8-2 2-8 (=Ne) 12 p+ 12 p+ 12 e- 10 e- 0 2+
Ions from Nonmetal Ions In ionic compounds, nonmetals in 15, 16, and 17 gain electrons from metals Nonmetal add electrons to achieve the octet arrangement Nonmetal ionic charge: 3-, 2-, or 1-
Fluoride Ion unpaired electron octet 1 - : F + e : F : 2-7 2-8 (= Ne) 9 p+ 9 p+ 9 e- 10 e- 0 1 - ionic charge
Ionic Bond Between atoms of metals and nonmetals with very different electro negativity Bond formed by transfer of electrons Produce charged ions all states. Conductors and have high melting point. Examples; NaCl, CaCl2, K2O
ionic bond
1). Ionic bond electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.
ionic bond
METALLIC BOND bond found in metals; holds metal atoms together very strongly
Metallic Bond Formed between atoms of metallic elements Electron cloud around atoms Good conductors at all states, lustrous, very high melting points Examples; Na, Fe, Al, Au, Co
Ionic Bond, A Sea of Electrons
Metals Form Alloys Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal. Examples are steel, brass, bronze and pewter.
Formula Weights Formula weight is the sum of the atomic masses. Example- CO2 Mass, C + O + O 12.011 + 15.994 + 15.994 43.999
Practice Compute the mass of the following compounds round to nearest tenth & state type of bond: NaCl; 23 + 35 = 58; Ionic Bond C2H6; 24 + 6 = 30; Covalent Bond Na(CO3)2; 23 + 2(12 + 3x16) = 123; Ionic & Covalent
Video NaCl Formation.mp4
ionic bond

More Related Content

ionic bond

  • 2. Atom the smallest unit of matter indivisible Helium atom
  • 3. electron shells a) Atomic number = number of Electrons b) Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells. a) Electron shells determine how an atom behaves when it encounters other atoms
  • 4. Electrons are placed in shells according to rules: 1) The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons.
  • 5. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to Gain 4 electrons Gain 3 electrons Gain 2 electrons
  • 6. Why are electrons important? 1) Elements have different electron configurations different electron configurations mean different levels of bonding
  • 8. Electron Dot Structures Symbols of atoms with dots to represent the valence- shell electrons 1 2 13 14 15 16 17 18 H He: Li Be B C N O : F :Ne : Na Mg Al Si P S :Cl :Ar :
  • 9. Chemical bonds: an attempt to fill electron shells 1. Ionic bonds 2. Covalent bonds 3. Metallic bonds
  • 10. IONIC BOND bond formed between two ions by the transfer of electrons
  • 11. Formation of Ions from Metals Ionic compounds result when metals react with nonmetals Metals lose electrons to match the number of valence electrons of their nearest noble gas Positive ions form when the number of electrons are less than the number of protons Group 1 metals 錚р ion 1+ Group 2 metals 錚р ion 2+ Group 13 metals 錚р ion 3+
  • 12. Formation of Sodium Ion Sodium atom Sodium ion Na e 錚эр Na + 2-8-1 2-8 ( = Ne) 11 p+ 11 p+ 11 e- 10 e- 0 1+
  • 13. Formation of Magnesium Ion Magnesium atom Magnesium ion Mg 2e 錚р Mg2+ 2-8-2 2-8 (=Ne) 12 p+ 12 p+ 12 e- 10 e- 0 2+
  • 14. Ions from Nonmetal Ions In ionic compounds, nonmetals in 15, 16, and 17 gain electrons from metals Nonmetal add electrons to achieve the octet arrangement Nonmetal ionic charge: 3-, 2-, or 1-
  • 15. Fluoride Ion unpaired electron octet 1 - : F + e : F : 2-7 2-8 (= Ne) 9 p+ 9 p+ 9 e- 10 e- 0 1 - ionic charge
  • 16. Ionic Bond Between atoms of metals and nonmetals with very different electro negativity Bond formed by transfer of electrons Produce charged ions all states. Conductors and have high melting point. Examples; NaCl, CaCl2, K2O
  • 18. 1). Ionic bond electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.
  • 20. METALLIC BOND bond found in metals; holds metal atoms together very strongly
  • 21. Metallic Bond Formed between atoms of metallic elements Electron cloud around atoms Good conductors at all states, lustrous, very high melting points Examples; Na, Fe, Al, Au, Co
  • 22. Ionic Bond, A Sea of Electrons
  • 23. Metals Form Alloys Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal. Examples are steel, brass, bronze and pewter.
  • 24. Formula Weights Formula weight is the sum of the atomic masses. Example- CO2 Mass, C + O + O 12.011 + 15.994 + 15.994 43.999
  • 25. Practice Compute the mass of the following compounds round to nearest tenth & state type of bond: NaCl; 23 + 35 = 58; Ionic Bond C2H6; 24 + 6 = 30; Covalent Bond Na(CO3)2; 23 + 2(12 + 3x16) = 123; Ionic & Covalent