Unit 2 - Chemistry: Compounds and the periodic table Flashcards
Non-metallic elements compound is called..
Covalent bonding
Non-metallic elements form non-ionic compounds using a different type of bonding called covalent bonding involving shared pairs of electrons.
Describe lithium, sodium and potassium in Group 1
A collection of relatively soft metals showing a trend in melting point and reaction with water. Reactivity and colour increases down the group.
All elements in group 1 react with water to form an alkali.
Describe transition elements
A collection of metals having high densities, high melting points and forming coloured compounds, and which, as elements and compounds, often act as catalysts.
Describe noble gases
Unreactive. Full outer electron shell.
Describe the composition of clean air
A mixture of 78% nitrogen, 21% oxygen and small quantities of noble gases, water vapour and carbon dioxide.
Describe the formation of carbon dioxide
- A product of complete combustion of carbon-containing substances
- A product of respiration
- A product of the reaction between an acid and a carbonate.
Relate the terms exothermic and endothermic to the temperature changes observed during chemical reactions
During all chemical reactions, an energy change occurs. In the reaction heat is either released or absorbed. When a reaction releases heat to the surroundings, we call that reaction an Exothermic Reaction. The reaction that absorbs energy from the surroundings are called Endothermic Reactions.
EXOTHERMIC
The reactants have more energy than the products here, so a small amount of energy is required to activate the reaction.
- Release of heat
- Energy needed for the reaction to occur is less than the total energy released.
- Extra energy is released, usually in the form of heat.
- The release of heat means that an exothermic reaction increases temperature of the surroundings.
ENDOTHERMIC
- Heat absorbs energy from the surroundings.
- Temperature of surroundings decreases during an endothermic reaction because energy from surroundings is required to drive the reaction, hence decreasing the temperature of the surroundings.
Demonstrate understanding that exothermic and endothermic changes relate to the transformation of chemical energy to heat (thermal energy), and vice versa.
Exothermic:
Chemical -> heat
Endothermic
Heat -> chemical
In order to actually start a reaction, a certain amount of energy will be provided to the reactants; We often call this the Energy of Activation because this energy is essentially required to start the reaction.
The energy here is used to break the bonds between the molecules of the atoms of the reactants. The bonds then subsequently rearrange and bond again, which releases energy.
However, if the energy provided to activate the energy is less than the energy released when the bonds form together, the reaction gave out more than it took/absorbed, which makes this a exothermic reaction. If the energy given to activate is more than the energy released during the bond formation, the reaction is endothermic.
The total energy change is called enthalpy.
Describe the formation of ions
If an atom loses or gains an electron we call it an ion.
An atom is pretty stable. It has an equal number of electrons and protons.
However, atoms often have the potential to become unstable. The truth is, most atoms don’t like to have outer electrons. If you look at the noble gases in group 8, they don’t have any outer electrons. The elements in group 1-7 all want to become like a noble gases in terms of electron configuration.
Describe the formation of ionic bonds between elements from group I and VII
Ionic Bonding is basically a process where a non-metal and metal each donate the appropriate number of electrons to each other to form a compound with a stable electron configuration.
Eg Na has an electron configuration of 2, 8, 1. It needs to lose one electron
Chloe has an electron configuration of 2, 8, 7 so it needs to gain one electron.
The overall charge should be 0
Explain the formation of ionic bonds between metallic and non-metallic elements
The IONIC BOND results as a balance between the force of attraction between opposite plus and minus charges of the ions and the force of repulsion between similar negative charges in the electron clouds. In crystalline compounds this net balance of forces is called the LATTICE ENERGY. Lattice energy is the energy released in the formation of an ionic compound.
Metals always form positive ions
Non-metals always form negative ions
Draw dot-and-cross diagrams to represent the sharing of electron pairs to form single covalent bonds in simple molecules, exemplified by H2, Cl2, H2O, CH4 and HCl.
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Use the symbols of the elements to write formulae of simple compounds
Some common chemical compounds H2O - water HCl - hydrochloric acid H2SO4 - sulphuric acid. NH4+ - ammonium NO3- - nitrate OH- - hydroxide
Deduce the formula of a simple compound from the relative numbers of atoms present
It is possible to work out the chemical formulae of a compound when given the elements present.
For example, if we are told that a certain compound contains both sodium and chlorine, we can deduce its formulae to be NaCl.
Eg Mg has 2 outer electrons, Chlorine needs 1 more outer electron
so MgCl2
Deduce the formula of a simple compound from a model or a diagrammatic representation
A simple way would be to simply count the number of electrons in each atom!
The red dots represent the electrons of the element on the left and the blue crosses represent the electrons of the element of the right.
Since the diagram features an ionic compound, we have to take in account the single electron given from the positive ion to complete its full outer shell.
In total, the element on the left has 11 red dots, or electrons; if we look at the periodic table, the element with 11 electrons is sodium.
Likewise, the element on the right has 17 crosses, or electrons. Using the periodic table, the element with 17 electrons is Chlorine
Determine the formula of an ionic compound from the charges on the ions present
Eg if element x has 3 outer electrons, and element y has 6 electrons (needs two). Then it would be X2Y3
To work out the formulae of an ionic compound using the ions present simply remember that the charge on any ionic compound must be neutral, or 0.
For example, we are told that a compound has Fe2+ ions present as well as Cl- ions.
Using that information, for every Fe2+ present in the compound there must be 2 Cl- ions to balance out the charge. Therefore, the formula of the ionic compound must be FeCl2.