Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
26 Cards in this Set
- Front
- Back
|
Properties of Ionic Compounds |
High melting and boiling points can conduct electricity when melted or dissolved in water often soluble in water strong intermolecular force |
|
|
Properties of simple molecular compounds |
low melting and boiling points mostly insoluble in water low electrical conductivity weak intermolecular force |
|
|
Properties of Giant Covalent compounds/structures |
High melting and boiling points no conductivity in water except graphite insoluble in water |
|
|
Element that reacts similar to (blank) |
same group different period |
|
|
how are the elements arranged? |
increasing atomic number |
|
|
Alkali metal and water equation |
2alkali metal (s) plus 2H2O(I) yields 2(alkali metal)OH(aq) plus H2(g) |
|
|
Define displacement reactions |
the halogen with the highest reactivity will take the metal from the halogen less reactive |
|
|
Uses of noble gases |
Helium- balloons Argon- tungsten light bulb Neon- advertising signs Krypton- lasers Xenon- lighthouse lamps |
|
|
How to find relative formula mass |
calculate with atomic mass |
|
|
describe diamond and graphite's structure |
Diamond- each carbon atom is covalently bonded to four other carbon atoms. Graphite- Each Carbon atom forms 3 strong covalent bonds. There are weak forces of attraction between the layers. |
|
|
What makes diamond a hard substance? |
Bonding is extremely strong. Every carbon atom is covalently bonded to four other carbon atoms. |
|
|
Why can Graphite conduct electricity? |
the fourth unbonded electron from each carbon atom is delocalised and so it can move along the layers |
|
|
why do Graphite and Diamond have high melting points? |
held together by strong covalent bonds |
|
|
Explain why diamond has a very high melting point |
each carbon atom is strong covalently bonded to four other carbon atoms forming a very strong lattice structure. A very high temperature is needed to break down the structure. |
|
|
what is relative atomic mass and relative formula mass? |
Atomic mass: mass of a mole of atoms of an element Relative formula mass: mass of the ions used for ionic compounds MR |
|
|
how to find the number of moles |
mass/relative atomic mass |
|
|
In a displacement reaction, what should be more reactive? |
solution |
|
|
DESCRIBE ALKALI METALS |
-soft -low melting points (decrease down the group) -low densities (float on water) (increase down the group) -reactivity increases down the group -react with water to produce an alkaline solution |
|
|
DESCRIBE HALOGENS |
-react with most metals to make salt -all exists as diatomic molecules -undergo displacement reactions -low solubility -little reaction with water -reactivity increases up the group |
|
|
describe the noble gases' trends in the periodic table as they go down |
1. atoms increase in size and mass 2. density of the mass increases 3. the boiling points increases |
|
|
one substance is an insulator, and the other is a good conductor of electricity |
graphite contains free electrons. They can move through the graphite, carrying charge from one place to another allowing graphite to conduct electricity. Diamond is an insulator because there are no free electrons or ions. |
|
|
Why does diamond have a higher melting point than carbon dioxide |
Diamond is a giant covalent structure, while carbon dioxide is simple molecular structure. Diamond has a higher melting point because their covalent bonds are strong, and contains many covalent bonds. Carbon dioxide has a lower melting point because they have weak intermolecular forces that break down easily. |
|
|
how to calculate relative molecular mass? |
take the weight of the atom and multiply it by percent abundance. Add that to the second atom's weight multiplied by the percent abundance. |
|
|
trends in halogens |
down the group: color gets deeper density increases boiling points increases reactivity decreases |
|
|
Color changes |
chlorine to bromide solution- orange Chlorine to iodide solution- red-brown Bromine to iodide solution- red/brown |
|
|
Color changes |
chlorine to bromide solution- orange Chlorine to iodide solution- red-brown Bromine to iodide solution- red/brown |
