I have to finish this full worksheet in 2 days and there is NO way I can finish without having the book the answers are from!!
ION FORMATION AND NAMING
V. Valence Electrons and Chemical Bonds:
A. A ____________________________ is the force that holds two atoms together.
B. There are _______ different types of chemical bonds. _________________________, ____________________, and ______________________________.
C. ______________________________- bonds that are formed due to the attraction of positive and negative forces, these are _________________________ forces.
1. A positively charged ion has ___________ one or more valence electrons and is called a/an _____________.
a) __________________ atoms are reactive because they LOSE valence electrons easily. The group 1 and 2 metals are the most reactive metals on the periodic table.
b) __________________ metals will lose _______ valence electron(s) and end up with a +1 charge and __________________ total valence electrons.
c) __________________ metals will lose _______ valence electron(s) and end up with a +2 charge and __________________ total valence electrons.
d) __________________ metals will lose _______ valence electron(s) and end up with a +3 charge and __________________ total valence electrons.
e) __________________ metals do not follow exactly the same rules because of the overlap of the d and f orbitals. They will still usually form ions with a ________ or ________ charge because they will lose 2 OR 3 electrons. These will form what is called a ________________________________ formation but there are different rules that they follow and we will not deal much with them.
2. A negatively charged ion has ___________ one or more valence electrons and is called a/an ____________.
a) ____________________ atoms are reactive because they GAIN electrons easily. The group 16 and 17 nonmetals are the most reactive nonmetals on the periodic table.
b) ____________________ will gain ________ valence electron(s) to end up with a -1 charge and ________ total valence electrons.
c) ____________________ (beginning with oxygen) will gain ________ valence electron(s) to end up with a -2 charge and ________ total valence electrons.
d) ____________________ (beginning with nitrogen) will gain ________ valence electron(s) to end up with a -3 charge and ________ total valence electrons.
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Name: ____________________________________
D. The formation of an ionic bond begins with a ______________ and an ______________ coming together to form an ionic compound. These will come together to balance the overall charges to _____________. E. EXAMPLE PROBLEM: Explain how an ionic compound forms from these elements: sodium and chlorine. ______________________________________________________________________________ _____________________________________________________________________________________ F. PRACTICE PROBLEMS: Explain how an ionic compound forms from these elements. 1. Sodium and nitrogen
2. lithium and oxygen
3. strontium and fluorine
4. aluminum and sulfur
G. The strong attractions among the positive and negative ions in an ionic compound result in the formation of a ___________________________________, which is a 3-D geometric arrangement of particles. In this way, each positive ion is surrounded by ______________ ions and each negative ion is surrounded by ___________________ ions.
H. Melting point, boiling point, and hardness are _________________ properties of matter that depend on how strongly the particles that make up the matter are attracted to each other. Another property, ______________________ or the ability to conduct electricity, depends on the availability of freely moving charged particles. In other words, ___________ ionic compounds will not conduct electricity, but _____________ or ionic solids that are dissolved in solution can. (These are called __________________)
1. Ionic bonds are __________________ so ionic crystals require a large amount of _______________ to be broken apart.
2. This means that ionic compounds will have ______________ melting points and boiling points. VI. Names and Formulas for Ionic Compounds
A. The chemical formula for an ionic compound is called a _________________________. It represents the simplest ratio of the ions involved.
➢ Remember that an ionic compound aims to have an overall charge of _______________. So if you combine magnesium and chlorine together:
○ magnesium- _______- would have a charge of _______
○ chlorine- ________- would have a charge of _______
○ You would have to have _______ magnesium(s) and ______ chlorine atom(s) to end up with an electrically neutral compound (overall charge of ________)
B. Most ionic compounds are _______________, meaning they have two different elements, but some atoms will form _____________________ ions, meaning there will only be one element as an ion. 1. The charge of a monatomic ion is equal to its _______________________________. 2. The oxidation number of an element equals the number of ___________________ that are transferred to or from the atom to form the ion.
3. This follows a rule called the “_____________________________”, where an atom is considered most stable when it has _______________ valence electrons, or an _________________. This is called a _______________________________________________________.
a) Noble gases are generally unreactive because they _______________________________________. b) Group 1 elements (beginning with _________________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
c) Group 2 elements (beginning with _________________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
d) Group 13 elements (beginning with _______________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
e) Group 14 elements (beginning with _________________) will ______________ or ______________ _______ electron(s) because it is the same going up or going down to end up with a full valence shell.
f) Group 15 elements (beginning with __________________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
g) Group 16 elements (beginning with ___________________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
h) Halogens (beginning with ___________________) will _____________ _______ electron(s) because it is easier to _________ ______ than it is to ____________ _______ to get a full valence electron shell, or an octet.
i) Noble gases (beginning with ___________________) will generally NOT ______________ or ________________ electrons because they already have a full valence shell.
C. Formula rules for binary ionic compounds:
1. In the chemical formula for any ionic compound, the symbol of the ________________ is always written first, followed by the ___________________.
2. _____________________________ (the little tiny numbers on the bottom) are used to say how many of each atom is in the formula unit.
3. If no subscript is written in the formula unit, the assumed number of atoms in that element is _______.
D. Formulas for polyatomic ions
1. Many ionic compounds contain _______________________________, which are ions made up of more than one atom. (On the back of your periodic table there is a list of polyatomic ions for you to reference, you will not need to memorize them, but it will help you if you do!)
2. A polyatomic ion acts as an ___________________________________ in a compound and its charge applies to the entire group of atoms, THUS the formula for a polyatomic compound follows the same rules used for a binary compound.
3. Because a polyatomic ion exists as a unit, we _________________ change the subscripts of the atoms _____________________ the ion. If more than one polyatomic ion is needed, place a set of __________________________ around the polyatomic formula and place the appropriate subscript __________________ of the parentheses.
E. Names for ions and ionic compounds
1. Name the ______________________ followed by the _________________. Remember that the cation is always written __________________ in the formula.
2. For monatomic cations, use ____________________________.
3. For monatomic anions, use the root of the element name, plus the suffix (ending) ______________.
4. To distinguish between multiple oxidation numbers of the same element, the name of the chemical formula must indicate the oxidation number of the ______________________. (This USUALLY only happens with the _________________________________________.) The oxidation number is written as a __________________________________ in parentheses after the name of the _______________.
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