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Ionic Bonds project

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by

Xochitl Silva

on 18 December 2012

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Transcript of Ionic Bonds project

Obstacle 1 Obstacle 2 Obstacle 3 Now you Know! 8.2 Vocabulary An Ionic compound is bounded by, crystal lattice. Crystal lattice is built up so positive ions are nearest to the negative ions this will form a solid Review Information About Ionic Bounds YAY!! Ionic Bonds By: Xochitl Silva
Ionic bonds form when valence electrons go to and atom and then another. Ionic bonds fill the outermost level of an atom, like a chemical bonds Forming Negative/Positive/Compounds Ions Ionic Compounds and the Properties Energy is needed to remove electrons from metal atoms. Energy is released as the nonmetal atoms gain electrons Ionic Bond: an attractive force between oppositely charged ions, which form when electrons are transferred from one atom to another
Ion: a charged particle that forms when an atom or a group of an atoms gains or loses one or more electrons
Crystal Lattice: The regular pattern in which a crystal is arranged
Forming Ionic Compounds: When a metal and a nonmetal combine in an ionic bond it forms a compound with different properties. The ionic bonds forms because the opposite charges of the ions cause the ions to stick together. Forming Positive bonds: During chemical changes ionic bonds pull electrons forms positive ions.
Forming Negative bonds: The ions that form and have more electrons than protons the ions are overall negative.
An atom is neutral because, the number of electrons equals the number of protons in an atom so they electric charges cancel each other out. A transfer in electrons in an atom changes the number of electrons in each atom. Positive and negative charges no longer cancel out and atoms become ions.If an ion has more protons than electrons it's a positive ion. Between ions and crystal lattice they form physical properties ions are brittle solids in room temperature.
These solids will break apart with a hit by a hammer the solids have high melting points
Any property of many ionic compounds have high solubility in water which means that the compounds will dissolve Ionic Bonding usually occurs between atoms of metals and nonmetals Ions of different elements can combine by forming ionic bonds Ionic compounds form solids by building up a repeating pattern called crystal lattice Metal atoms and loss of electrons/ Energy needed to remove electrons The elements in Group 1 and 2 react easily because, the energy needed to remove electrons from their atoms are to small, when and atom loses electrons energy is needed to overcome the attraction of electrons to the protons. So, only ions, and not atoms, of the elements are found in nature, in ionic bonding energy is needed Atoms of most metals have few electrons in their outermost energy level, when metal atoms bond with other atoms they tend to lose valence electron to form positive ions, when an atom loses electrons to another atom it becomes an ion Thank you! An example of calculating charge in a sodium ion is it has 11 protons and 10 electrons, so you would add (11+) and (10-) to get a charge of 1+ Forming Ionic Compounds: When a metal and a nonmetal combine in an ionic bond it forms a compound with different properties. The ionic bonds forms because the opposite charges of the ions cause the ions to stick together. Mini Test! How do ionic bonds form? What is a property of an ionic compound?
A) crystal lattice
B) high solubility-in water
C) loose electrons
D)gain electrons What happens when an atom looses electrons? Why is an atom neutral? If an ion has more protons than electrons is it a positive ion? True or False? Is energy needed to remove electrons from metal atoms? True or False? Charged Particles Forming Ionic Bonds How do you form a positive ion? Ionic compounds form solids by,
A) very high boiling points
B) oppositely charged electrons
C) building up a crystal lattice Is less energy needed to take electrons from metal atoms? True or False? It takes less energy to take electrons from metals than nonmetals Atoms of most metals have few electrons? True or False?
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