Ionic and Covalent Bonding
Ionic and covalent bonding is involved when the atoms of an element
chemically combine to make their outer shells full and to make the
atoms stable.
The first type of bonding you can get is ionic bonding. Electrons are
transferred from one atom to another to try and create full outer
shells, this gain and loss of electrons on the atoms results in
positive and negative ions. In these compounds you get electrostatic
force, this is the force/attraction that occurs between the positive
and negative ions that hold the compound together. This type of
bonding takes place between metals and non-metals. The metals lose
electrons and form cations, whereas the non-metals gain electrons and
form anions.
Each energy sub level is made up of orbitals. Every one can hold a
different number of orbitals, these sub-levels are known as S, P, D
and F. when the S and P block elements lose or gain electrons to
become ions they fill their outer shells to get the electronic
structure of a noble gas, however this structure doesn’t apply to most
of the positive ions formed from the transition metals.
Ionic compounds exist as a regular arrangement of ions in a giant
covalent lattice. It is very hard to overcome the strong forces
between them known as the electrostatic force, this means that ionic
compounds are generally solid and they have a very high melting and
boiling points as they need a lot of energy to overcome the
electrostatic force. The bigger the charge on the atom and the smaller
the atom, the bigger the electrostatic force.
In simple ionic compounds the positive ion is often much smaller than
the negati...
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...e larger the strength of the Wan de Waal forces. The
bigger the forces are between the molecules the more energy is needed
to overcome them, giving the substance and higher melting and boiling
point.
There is another type of bonding and this is called metallic bonding,
this type of bonding is the force of attraction between the
delocalised electrons and the positive centres. The atoms of the
elements are packed so closely together that some of their electrons
begin to wander among the nuclei rather than orbiting the nucleus of a
single atom. As the charge on the positive centre and the number of
mobile electrons per atom both increase and the size of the positive
centre decreases the strength of the metallic bond increases. As they
have free electrons they conduct electricity very well in solid and
liquid states.
This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed.
Covalent compounds are formed when two or more non-metals react together. The covalent compound is actually made of molecules, and the name given depends on the structure of these molecules. Prefixes, like di- for two, tri- for three, tetra- for four, and so forth, are frequently used. Thus, NO2 is nitrogen dioxide and N2O4 is dinitrogen
Metals contain a sea of electrons (which are negatively charged) and which flow throughout the metal. This is what allows electric current to flow so well in all metals. An electrode is a component of an electric circuit that connects the wiring of the circuit to a gas or electrolyte. A compound that conducts in a solution is called an electrolyte. The electrically positive electrode is called the anode and the negative electrode the cathode.
The Pauli exclusion principle is defined by Dr. Steven S. Zumdahl, "In a given atom no two electrons can have the same set of four quantum numbers." Due to this principle, only two electrons can inhabit a single energy level. The electrons that share the same energy level have opposite intrinsic angular momentums which is more commonly known as "spin". To determine the direction of the spin the angular momentum vector is analyzed.
Hydrogen sulphide has a boiling point of -82 degrees Celsius and a melting point of -60 degrees Celsius. There are 2 hydrogen and 1 sulphide molecule. Simple molecule’s which are covalent have lower melting and boiling points as they do not need too much energy to separate the bonds because they are as polarised as water. In hydrogen sulphide the intermolecular forces are known as Dipole-Dipole forces which are less powerful than hydrogen bonding which is in water therefore water has the strongest bond compared to hydrogen chloride and hydrogen sulphide. Water is more electronegative than hydrogen chloride and hydrogen sulphide because there are more molecules in water which are drawn together however in hydrogen sulphide there are less molecules
It involves collisions between the free electrons, the fixed. particles of the metal, other free electrons and impurities. These collisions convert some of the energy that the free electrons are. carrying heat, which means that electrical energy is lost. Apparatus: I will be using an Ammeter.
Because they repel they are as far from each other as possible. The two electrons in each of the oxygen-hydrogen bond are not shared equally. They are more strongly attracted to the oxygen. The bond is polar, it has a 'negative part' (the oxygen) and a 'positive part' (the hydrogen).The hydrogen bond is very weak, about ten times weaker than a single covalent bond.
Anion gap is the difference of anion level and cation level within organism body fluid. The common cation that being measured are sodium ion and potassium ion, but potassium ion usually not included within the calculation due to very low amount within human body fluid (Emmett and Narins, 1977, pp. 38). The common anions used in the calculation of anion gap are chloride ion and bicarbonate ion. The calculation of anion gap as following:
From the unit of chemistry in grade ten science, the students have learned many things from different types of elements in the chart all the way to how each element impacts the daily life each student or even adult lives in. Some of the things I as a student have learned include how to draw the different elements in a bohr rutherford diagram, balancing chemical equations, types of chemical reactions, and even information about the different types of acids and bases. Although there were many other things in the unit, these four definately helped me learn about chemistry in a more in-depth way, as well as teaching me something very new since these were some things a few of the students had never done in the previous years. Learning this in the classroom has really opened my eyes to the world in which we live in today, many times I leave the house on a cold day and as I look upon the cold water becoming ice or even the snow falling down, I know how it is happening, why it is happening, and I can even picture the molecules solidifying as we had seen in class with many different diagrams.
...ubstances that have different properties than the properties of the reactants (blue book). Most atoms form bonds with valence electrons only, which means the number of valence electrons determines if an atom will form a bond (eight electrons are usually unreactive, while fewer than eight tend to bond more often). Atoms bond to fill their outermost energy level. They would either lose share or gain an electron. In baking soda and vinegar, you may be wondering what bonding has to do with a chemical reaction. Well, in order for a chemical reaction to take place a bond must be broken. This happens because molecules are always moving which means if they bump with enough energy, the bond will break. The atoms then rearrange and new bonds form to make new substances (blue book). So behind the aesthetic view of the “white fizz,” there is always a scientific explanation.
The Periodic Table of Elements is commonly used today when studying elements. This table’s history begins in ancient times when Greek scientists first started discovering different elements. Over the years, many different forms of the periodic table have been made which set the basis for the modern table we use today. This table includes over 100 elements and are arranged by groups and periods. Groups being vertical columns and periods being horizontal columns. With all of the research conducted over the years and the organization of this table, it is easy to use when needed.
Solids, liquids, and gases are the three main, or fundamental phases of matter. Each one has a different density and a different level of stability. What determines the stability of each phase is the bond between it's atoms. The tighter the bond between it's atoms the more stable that phase of matter is. Solids are the most stable form of matter, followed by liquids, and then gases.
If the distance between the two electrodes is smaller, the copper ions need less energy to flow from the anode to the cathode
From these properties of bonds we will see that there are two fundamental types of bonds--covalent and ionic. Covalent bonding represents a situation of about equal sharing of the electrons between nuclei in the bond. Covalent bonds are formed between atoms of approximately equal electronegativity. Because each atom has near equal pull for the electrons in the bond, the electrons are not completely transferred from one atom to another. When the difference in electronegativity between the two atoms in a bond is large, the more electronegative atom can strip an electron off of the less electronegative one to form a negatively charged anion and a positively charged cation. The two ions are held together in an ionic bond because the oppositely charged ions attract each other as described by Coulomb's Law.
In chemistry, metals compose a great number of the periodic table elements. Each metal has its own characteristic mass,