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Ionic bonding report
Characteristics of ionic bonding and covalent
Essay ionic bonding
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Chemical notes on bonding
Ionic bonding
- This occurs between metals and non metals
- Fe2+/3+, Cu+/2+, Zn2+, No3-
- Metals loose electrons, non metals gain electrons.
- Ionic compounds conduct electricity when dissolved, but not when solid, they also have high m & b points due to strong giant 3d lattice. They are also soluble in water as they have a charge
- Metal atoms always form positive charged electrons while non metals from negatively charged electrons
Metallic Bonding
- They conduct electricity due to a sea of delocalised electrons
- They have a lattice of positive atoms.
- Transition metals contribute both S and D electrons in the sea of electrons
- The attraction is between the ions and mobile valence electrons and not between the layers, this means they can bend over each other
- The large the number of valence electrons and the smaller the atoms and the stronger the metallic bonding
Covalent bonding
- Between non metals with high electron values
- Can have single, double, or triple bonds
Bond strength
C – C: single bond, longest type of bond (154) however is the easiest to break (346)
C=C: double bond, second longest bond (134) and second hardest to break (598)
C=C: triple bond, smallest bond (121) however is the hardest to break (837)
Predicting the type of bonding
(1) From electronegativity
Electronegativity is the strength of an element/atom to pull electrons towards itself. Metals have a very low electronegativity as they lose electrons in ionic bonding, however non metals have a higher electronegativity as they gain electrons in ionic bonding.
(2) From position in the periodic table
Metal + non metal = ionic bonding
Non metal + non metal = covalent bonding
Simple molecular structure
Molecular covalent bonds have low m & b points because of weak intermolecular forces called Van Der Waals forces. (more on this later)
Giant covalent structures
Diamond and graphite both have these structures but they are very different. They both have a giant lattice with strong covalent bonds, in the case of Diamond it is 3d and very hard to break in any way, however with graphite it is only 2d so can be broken if cracked in a certain way. These structures have very high melting and boiling points.
Buckminsterfullerere
A family of ball shaped C-molecules in which there are around 60 atoms which are found in ball shapes. Uses are being investigated in nano-thecnology. These substances are soluble in non-polar solvents
Polar bonds
The larger the difference in electronegativity the greater the strength of the polar bond.
Now the hard stuff
A weak peak was at a position between 1600-1620 cm-1 can also be seem in the IR, which was likely to be aromatic C=C functional group that was from two benzene rings attached to alkynes. On the other hand, the IR spectrum of the experimental diphenylacetylene resulted in 4 peaks. The first peak was strong and broad at the position of 3359.26 cm-1, which was most likely to be OH bond. The OH bond appeared in the spectrum because of the residue left from ethanol that was used to clean the product at the end of recrystallization process. It might also be from the water that was trapped in the crystal since the solution was put in ice bath during the recrystallization process. The second peak was weak, but sharp. It was at the position of 3062.93 cm-1, which indicated that C-H (sp2) was presence in the compound. The group was likely from the C-H bonds in the benzene ring attached to the alkyne. The remaining peaks were weak and at positions of 1637.48 and 1599.15 cm-1, respectively. This showed that the compound had aromatic C=C function groups, which was from the benzene rings. Overall, by looking at the functional groups presented in the compound, one can assume that the compound consisted of diphenylacetelene and ethanol or
The bond energy is a measure of the amount of energy needed to break apart one mole of covalently bonded gases. The SI units used to describe bond energy are kilojoules per mole of bonds (kJ/mol).
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 bonds of reactions can only be broken when molecules of certain kinetic energies collide.
In the last 30 years, data obtained from spectrometric measurements, Xray and electron diffraction studies, and other experiments have yielded precise information about bond distances, angles, and energies. In many cases, the data confirmed conclusions reached earlier. In other cases, valuable new insights were acquired. Structure theory has advanced far beyond the simple electron dot representations and now rests securely on the foundations of quantum and wave mechanics. Although problems involving only simple molecules can now be solved with mathematical rigor, approximations such as the valence bond theory and the molecular orbital theory are very successful in giving results that agree with experimental measurements.
Regarding, the copper and sodium chloride, no visible change occurred after 5 minutes had passed. The copper metal remained at the bottom of the test tube undeterred by the NaCl. There may not have been a reaction because copper is lower on the reactivity series than sodium.
Negative ions are created when atoms have a high electronegative charge when they are bonded by covalent bonds to atoms which have a smaller electronegative charge share more electrons compared to the other atom. That is why a tiny negative charge on the atom; is more electronegative and a tiny positive charge which is on the atom ( that it is connected to the molecule) this bond is called a polar covalent bond. The elements electronegativity rises from the top of the groups in the periodic table and from the left to the right across the period in the periodic table. Hydrogen is an atom however it is not as electronegative as oxygen because hydrogen has an electronegativity value of 2.0 on the Pauling scale but oxygen has an electronegativity value of 3. 5 therefore the difference between these two values is 3.5 -2=1.5 which means that the difference in the electronegativity value for hydrogen and oxygen is 1.5. This difference is the reason why water is a polar molecule specifically a polar covalent molecule. The electronegativity value for sulphur is 2.58 on the Pauling scale of electronegativity this suggest that sulphur is also an electronegative molecule Chloride has an electronegativity value of
23. S. Alwarappan, S. Boyapalle, A. Kumar, C.-Z. Li and S. Mohapatra, J. Phys. Chem. C, 2012, 116, 6556–6559
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A Diamond is one of the two natural minerals that are produced from carbon. The other mineral is Graphite. Even though both of these minerals are produced from the same element ,carbon, they have totally different characteristics. One of the most obvious difference is that Diamond is hard and Graphite is soft. The Diamond is considered to be the most hardest substance found in nature. It scores a perfect ten in hardness. Because of its hardness a tiny Diamond is used as a cutting and drilling tool in industry. Even the Greeks called the Diamond “adamas” which means unconquerable. Diamonds also conducts heat better than any other mineral .
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.
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ike the other alkali metals, lithium has a single valence electron that is easily given up to form a cation. Because of this, it is a good conductor of heat and electricity as well as a highly reactive element, though the least reactive of the alkali metals. Lithium's low reactivity compared to other alkali metals is due to the proximity of its valence electron to its nucleus (the remaining two electrons are in lithium's 1s orbital and are much lower in energy, and therefore they do not participate in chemical bonds).
There are formulas to calculate electrical conductivity and resistivity. Conductivity is defined as the inverse of resistivity (a high conductivity means a low resistance), I=V/R or current equals voltage over resistance. This is known as Ohm’s Law. Electrical resistance is calculated by the formula, R=V/I or resistance equals voltage over current. Ohm’s law however does not hold true if temperature changes. Materials that obey Ohm’s law are known as ohmic or linear because the potential difference across it varies linearly with the current. In addition, whether or not a material obeys Ohm’s law its resistance can be described in bulk resistivity. Furthermore, over sizable ranges of temperature, this temperature depe...
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