#1) Draw the following ions using a Bohr diagram:
b)oxygen: i got [oxygen:2)8)]-2 (the -2 is an exponent) but the answer said [oxygen: 2)8)8)]-2...is this right?
d)fluorine: i got [fluorine:2)8)]-1 and the book says [fluorine: 2)8)8)]-1..again, is the book making a mistake?
#8)Using Lewis structures, draw the formation of the following ionic bond and write its chemical formula: magnesium and phosphorus.
Your book is wrong.
Thanks, but what about the next question:
#8)Using Lewis structures, draw the formation of the following ionic bond and write its chemical formula: magnesium and phosphorus
#1) To draw the Bohr diagram for an ion, we need to first determine the number of electrons in the ion. The atomic number of oxygen is 8, which means it has 8 electrons in its neutral state.
To determine how many electrons an ion has, we consider the charge on the ion. In this case, you mentioned that the oxygen ion has a charge of -2. This means that the ion has gained 2 extra electrons.
To draw the Bohr diagram, we represent each electron as a dot or a cross around the symbol of the element.
For oxygen (O), we start by drawing two electrons in the first energy level (closest to the nucleus), and then eight electrons in the second energy level. However, since we have a charge of -2, we add two more electrons to represent the extra electrons gained by the ion. Therefore, the correct Bohr diagram should be [oxygen: 2)8)8)]-2.
Similarly, for fluorine (F), its atomic number is 9, so it has 9 electrons in its neutral state. You mentioned that the fluorine ion has a charge of -1. This means the ion has gained one extra electron. So, the correct Bohr diagram for fluorine should be [fluorine: 2)7)]-1.
#8) To draw the Lewis structure and find the chemical formula for the ionic bond between magnesium (Mg) and phosphorus (P), we first need to determine the number of valence electrons for each element. Magnesium is in group 2 of the periodic table, so it has 2 valence electrons. Phosphorus is in group 15, so it has 5 valence electrons.
To form an ionic bond, magnesium needs to lose 2 electrons to fulfill the octet rule, while phosphorus needs to gain 3 electrons.
The Lewis structure for magnesium will show the symbol "Mg" with 2 dots around it representing its 2 valence electrons. The Lewis structure for phosphorus will show the symbol "P" with 5 dots representing its 5 valence electrons.
To form an ionic bond, magnesium will transfer its 2 valence electrons to phosphorus, resulting in both atoms achieving a stable electron configuration. After the transfer, magnesium will have a charge of +2 (lost 2 electrons) and phosphorus will have a charge of -3 (gained 3 electrons).
The chemical formula is determined by balancing the charges of the ions involved. In this case, since magnesium is +2 and phosphorus is -3, we can use the cross-multiplication method. The chemical formula is Mg3P2.
So, the Lewis structure for the ionic bond between magnesium and phosphorus is:
[Mg]2+ [P]3- with arrows representing the transfer of electrons.
The chemical formula is Mg3P2.