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Ionic and Metallic bonding Chapter Review (Evans)

Terms in this set (29)

Anion
A negatively charged ion
Cation
A positively charged ion
Crystal lattice
The regular repeating arrangement of ions in an ionic compound
Delocalized electron
An electron that continues to to be transferred to different metal elements
Ductile
The ability for metal to be drawn into wire
Electron transfer
When electrons transfer from different metal elements consistently
Electronegativity
Energy required to gain a valence electron
Halide ion
Halogen atom bearing a negative charge
Ionic compound
Composed of billions of cations and anions electrostatically attracted to eachother
Ionization energy
Energy required to lose a valance electron
Lewis Dot Structure
Diagram showing electrons moving from one element to another
Malleable
The ability for metal to be pounded
Metallic bond
Mobile sea of delocalized electrons which are mutually attracted to and shared by a cluster of metal cations
Octet rule
When an atom is stable it will have 8 electrons on the valence shell
Valence electron
Electron on the outer shell
Valence shell
The outer shell on an atom
1. Ba, Cl
2. Mg, Mg
3. Ni, O
4. Fe, S
5. P, Br
6. Bi, F
7. Al, Al
8. Mn, I
9. Cu, Zn
1.ionic
2. Metallic
3. Ionic
4. Ionic
5. Covalent
6. Metallic
7. Metallic
8. Ionic
9. Metallic
1. AlBr3
2. NaF
3. CaO
4. Na+
5. Lithium Fluoride
6. Barium Phosphide
7. Calcium Iodide
8. Phosphide Ion
1. Aluminum Bromide
2. Sodium Fluoride
3. Calcium oxide
4. Sodium Ion
5. LiF
6. Ba3P2
7. CaI2
8. P-3
Explain how an ionic bond forms. In your answer, indicate which atom donates the electron and which atom excepts it and why?
A metal and a non metal attract because they have opposite charges and the cation wants to donate an electron to the anion in order to make them stable
When an atom becomes a cation, it gets smaller; when an atom becomes an anion it gets larger explain why.
The cation donates electrons it loses a shell and it adds electrons to the anion completing a shell making the cation smaller and anion larger
Explain why ionic compounds have the following properties
A) high melting points
B) brittle as solids
C) dissolve in water
D) definite crystalline structure
E) conduct electricity in the molten state or when dissolved in water
A) it takes such a high amount of energy to break them so that's why the melting point is so high
B) the crystal structure the bonds are so strong that if it shifts and like charges are next to each other it will repel and explode
C) when it goes into water it bonds with the covalent bond water and then separates the electrons from it making it dissolve.
D) ions are arranged within the lattice in such a way as to maximize the separation of like charged and minimize the separation of oppositely charged ions
E) since when it dissolves in water are forming ions and electrons are moving giving it the ability to conduct electricity
Explain how and why metallic bonds form?
Metallic bonds form when cation metals have - electrons that delocalize and transfer to metals
Explain why the following are properties of metals
A)malleable and ductile
B) good conductors of electricity
A) the electrons and cations shift there position so they can be drawn into wire or pounded
B) since the metals can be pounded into different shapes heat can flow through them easily
An ionic bond is an _____________force that holds cations and anions together
Electrostatic
What would be the charge on Mg when it becomes a cation?
Positive
What would be the charge of S when it becomes an anion?
Negative
Does an element become a cation by gaining or losing electrons?
Losing
Does an element become an anion by gaining or losing electrons?
Gaining
Are electrons in an ionic bond shared?
No they are not shared they are transferring electrons from a metal to a non metal.
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