Chapter 7 Outline
Ionic and Metallic Bonding
- Section 7.1 – Ions
- are the electrons in the ______occupied energy level.
- are the only electrons involved in ______.
- Elements in the same have the same ______of valence electrons.
- are diagrams that show the of the element surrounded by the valence electrons are .
- Practice Problems
- Write the electron dot structure for the following elements:
P ArMgHe
- The states that atoms tend to achieve a configuration when they have valence electrons.
- tend to electrons to achieve noble-gas configuration. tend to ______electrons to achieve noble-gas configuration.
- A ion is a ion that has ______electrons.
- When writing the for a cation, write the electron configuration for the ______and then subtract the electrons from the ______energy level.
- When you name a , the name of the ______does not change. Ex: Ca+2 =
- Sample Problem
- Write the electron configuration and name for the following:
Sr2+
Fe+3
- Practice Problems
- Write the electron configurations and the name for the following:
Zn+2
Na+
- are charged ions that have ______electrons.
- When writing the for anions, write the electron configuration for the and then the correct number of electrons.
- When naming an , you change the ending of the element to . Ex: Cl- =
- Sample Problems
- Write the electron configuration and name for the following:
P-3
F-
- Practice Problems
- Write the electron configuration and name for the following:
Br-
S-2
- Section 7.1 Assessment
- How can you determine the number of valence electrons in an atom of a representative element?
- Atoms of which elements tend to gain electrons? Atoms of which elements tend to lose electrons?
- How do cations form?
- How do anions form?
- How many valence electrons are in each atom?
- Potassium
- Carbon
- Magnesium
- Oxygen
- Draw the electron dot structure for each element in question 5.
- How many electrons will each element gain or lose in forming an ion?
a. calcium
b. fluorine
c. aluminum
d. oxygen
- Write the name and symbol of the ion formed when
a. a potassium atom loses one electron.
b. a zinc atom gains one electron
c. a fluorine atom gains one electron
- Write the electron configuration of Cd+2.
- Section 7.2 – Ionic Bonds and Ionic Compounds
- Compounds composed of are called .
- Although they are composed of , ionic compounds are electrically .
- The that hold ions together are called .
- A shows the kinds and ______of atoms in the smallest representative unit of a substance.
- A is the lowest ______
______of ions in an ionic compound.
- When you charges to write the ______for an ionic compound, you must make the charge and charge equal by adding subscripts.
- The must be in the ratio to be correct.
- Sample Problems
- Write the formula for the compound formed between the following elements.
Potassium and oxygen
Magnesium and nitrogen
- Practice Problems
- Write the formula for the compound when the following elements combine.
Potassium and iodine
Aluminum and oxygen
Calcium and chlorine
Barium and sulfur
- are a group of atoms with an overall .
- When charges for polyatomic ions, you follow the same of cancelling the + and – charge.
- However, if you need to add a to a polyatomic ion, then you have to put the polyatomic ion in . Ex: Ca(NO3)2
- Sample Problems
- Write the formula for the compound when the following ions combine:
Sodium and phosphate
Ammonium nitride
Aluminum carbonate
- Practice Problems
- Write the formula for the compound when the following ions combine:
Barium nitrate
Lithium phosphate
Strontium sulfite
- Properties of ionic compounds include the following:
- solids
- High points
- Conduct when molten or aqueous
- Made of ______
- Made of ______
- Made of ______
- A is a substance with a repeating arrangement of particles called the .
- The of an ion is the number ions of charge that surround the in a crystal.
- Section 7.2 Assessment
- How can you describe the electrical charge of an ionic compound?
- What properties characterize ionic compounds?
- Write the correct chemical formula for the compounds formed by each pair of ions.
K+, S-2
Ca+2, O-2
Na+, O-2
Al+3, N-3
- Write formulas for each compound.
barium chloride
Magnesium oxide
Lithium oxide
Calcium fluoride
- Which pairs of elements are likely to form ionic compounds?
Cl, Br
Li, Cl
K, He
I, Na
- Section 7.3 – Bonding in Metals
- The of metal atoms can be modeled as a .
- consist of the attraction of the free-floating valence for the positively charged .
- are good conductors and ______because of their electrons.
- are the most crystals because they contain type of element.
- An is a mixture with ______properties.
- A is made when atoms of one metal atoms of another metal.
- An is made when ______metal atoms are inserted in larger metal atoms.
- Section 7.3 Assessment
- How do chemists model the valence electrons in metal atoms?
- How can you describe the arrangement of atoms in metals?
- Why are alloys more useful than pure metals?
- Describe what is meant by ductile and malleable.
- Section 9.1 – Naming with Regular Metals
- A is a single atom with a charge. Ex:
- When naming a , the name of the element does not . Ex: K+ =
- When naming an , the ending of the element changes to . Ex: O-2 =
- A ______is a group of atoms with an overall charge. Ex: SO4-2
- Most polyatomic ions end in or . The ending does not change when naming a compound (unless it is an which we will talk about later).
- The suffix indicates that the polyatomic ion contains one more than the polyatomic ion with the suffix. (Ex: sulfate = SO4-2, sulfite = SO3-2)
- The are located in groups 1 and 2 (except for ). is also a regular metal.
- When naming a compound that starts with a ______
______, you name the (cation) and add ____ to the nonmetal (anion). Ex: NaCl =
- If the anion is a , then you do not change the . Ex: CaCO3 =
- Sample Problems
- Name the following compounds:
Na2O
AlBr3
Li2SO4
- Practice Problems
- Name the following compounds:
LiNO3
Ca2(PO4)3
(NH4)2O
- When writing the of a compound that starts with a regular metal, you must ______
______.
- Ex: aluminum bromide
- Sample Problems
- Write the formula for the following compounds:
Aluminum chloride
Calcium acetate
Lithium fluoride
- Practice Problems
- Write the formula for the following compounds:
Calcium carbonate
Aluminum oxide
Cesium oxalate
- Section 9.1 Assessment
- What are the usual ending for the names of polyatomic ions?
- How does a polyatomic ion differ from a monatomic ion?
- Write the formula for these binary compounds.
Beryllium chloride
Cesium sulfide
Sodium iodide
Strontium oxide
- Write the formula for these compounds.
- sodium perchlorate
- magnesium hydrogen carbonate
- calcium acetate
- Identify any incorrect formulas. Explain your answer.
- Mg2(SO4)3
- Rb3As
- BeCl3
- NaF
- Section 9.2 – Naming with Transition Metals
- can have charges, so you cannot tell the charge based on the it is in.
- Since transition metals can have charges, we use a to indicate the charge.
- Review of Roman Numerals
1 =
2 =
3 =
4 =
5 =
- **You should not use a roman numeral over 5.
- When compounds that start with a transition metal, you should charges to figure out the of the transition metal.
- Remember add to the anion if it is not a polyatomic ion.
- Ex: CuO
- Sample Problems
- Write the names for the following:
Cu2O
FeCl3
PbSO4
- Practice Problems
- Write the name of the following:
PbS2
Zn(C2H3O2)2
Ag3PO3
- For the naming system for ______the old names are used with the suffix –ic or –ous.
Ion / Old Name / Ion / Old Name
Fe3+ / ferric / Sn4+ / stannic
Fe2+ / ferrous / Sn2+ / stannous
Cu2+ / cupric / Pb4+ / plumbic
Cu+ / cuprous / Pb2+ / plumbous
Co3+ / cobaltic / Hg2+ / mercuric
Co2+ / cobaltous / Hg22+ / mercurous
- The ending indicates a charge, and the ending indicates a charge.
- When writing the for a compound, you figure out the for the transition metal and then find the old name on the .
- Ex: FeS
Fe+2S-2
Fe+2 = ferrous
FeS = ferrous sulfide
- Practice Problems
- Write the old names for the following:
Cu3P
Fe(NO3)3
PbS
- When writing the for a compound that starts with a , you must ______.
- Ex: vanadium (V) fluoride
- REMEMBER THE ROMAN NUMERAL IS THE , NOT THE !!!!!!!!!!!!!!!!
- Sample Problems
- Write the formula for the following:
Tin (II) permanganate
Mercury (I) oxide
Cobaltic carbonate
- Practice Problems
- Write the formula for the following:
Gold (II) iodide
Vanadium (IV) nitrite
ferrous chromate
- Section 9.2 Assessment
- Write the formula for chromium (III) nitrite.