Elements
Compounds
Ionic
Covalent
Properties
100
Which subatomic particle within an atom of an element are responsible for that element's chemical properties?
the electrons
100
Why do elements form compounds?
In order to become stable - have 8 valence electrons - an octet
100
Describe what happens in an ionic bond in terms of electrons.
Electrons are transferred from a metal to a nonmetal forming ions (+ and -) held together by attractive forces that result from the opposing charges.
100
What types of elements form covalent bonds?
nonmetals
100
Is pure water (H2O) able to conduct electricity? Why?
No, it is a covalent compound - no free ions which are necessary to carry electric current.
200
Which group of elements on the periodic table are considered the most stable and Why?
Group 8, Noble gases because they have a full outer valence shell (an octet)
200
What type of compound would a metal and a non metal form?
Ionic Compound
200
Why are ionic compounds neutral overall when they are made up of positive and negatively charged ions?
The positive and negative ions are equal but opposite and therefore will cancel each other out.
200
Identify 2 elements that could potentially form a covalent bond.
any 2 nonmetals (including Hydrogen)
200
Which of the following compounds would be most soluble in water, Calcium oxide, Carbon Monoxide, or Oxygen gas (O2)?
calcium oxide
300
Identify an element discussed in this chapter that is harmful to humans when encountered in its elemental form, but non-hazardous when in a compound
any alkali metal; chlorine
300
What type of compound involves a sharing of electrons? Provide an example of this type of compound.
A covalent compound - any two nonmetals together ie: H2O, CO2, N2, H2, HI etc.
300
What word can be used to describe the structure of an ionic compound?
crystal or crystalline
300
What is the other term that is commonly used when referring to a covalent compound?
molecule
300
Why do ionic compounds have higher melting points than covalent compounds?
Because ionic bonds are stringer than covalent bonds, therefore more heat (energy) is required to break ionic bonds.
400
Which types of elements tend to lose electrons when bonding ionically and become positively charged ions?
Metals
400
Explain how an ionic bond is formed and how it is held together.
Electron(s) are transferred from a metal to a nonmetal forming a positive ion and a negative ion, they are held together by the attractive force between the (+) charged and the (-) charged ions.
400
What are the names we use for positive and negative ions? You must state which name is for which ion.
(+) cation (-) anion
400
Which are stronger, ionic or covalent bonds?
ionic bonds
400
Why are ionic compounds able to conduct electricity when melted or dissolved in water?
Because in those states, their ions are free to move around and it is the free moving ions that allow for conductivity.
500
Why are the properties of compounds often times vastly different than the properties of the elements that make them up?
Because, when elements chemically combine to form compounds, their electron configurations are rearranged and thus their compositions are changed, resulting in different physical and chemical properties.
500
If aluminum were to bond ionically with nitrogen, explain which element would gain electrons and which would lose electrons and how many electrons would be gained/lost.
Aluminum would lose 3 and nitrogen would gain 3.
500
If Calcium became an ion, it would have the same electron configuration as which noble gas?
Argon
500
Which of the following is not a covalent compound? hydrogen sulfide; carbon monoxide; tin iodide; silicon dioxide
tin iodide
500
You are given an unknown white substance to identify. After some experimentation you determine that it is soluble in water and that it conducts electricity when dissolved in water. Is this substance more likely to be ionic or covalent?
Ionic
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