Global Warming is a threat to the survival of Polar Bears

The concept of global warming envisages the warming of the atmospheric layer where the volume of the Carbon dioxide gas is tremendously increased. The state of growing up of Carbon-di-oxide exists due to shortage of plants and trees and green house effects. This global warming is a threat to the survival of polar bears of arctic regions. Polar bears are ferocious and killer animals but they have a vital role to keep the environment free from pollutions. And as such our environment remains healthy and upkeep due to survival of such mischievous animals on artic regions..

We are conversant that the ultraviolet ray emit from the sun and due to tremendous increase in atmospheric layer, ozone layer is licked and ultraviolet rays pass through he ozone layer and fall into the surface of the earth.. As a result, the earth’s surface layer is warmed up and ultimately, the height of the sea level goes up. In this respect, the modern scientists believe that one day, the earth will remain inundated under water. Due to the global warming taking place into the arctic region, ice melts down and as such polar bears find difficulties to survive on earth. In this case, some polar bears are found missing and somehow, some survive through continuous suffering and painstaking efforts. The polar bears who somehow survive find less food during this time. When their hibernation starts, they cannot be able to save sufficient food reserves in the form of fat inside their bodies. Thus, due to colossal effects of global warming, polar bears are being died out day by day.

Polar bears are of great use to usas it destroys poisonous insects and other dust particles which are wasted away by tremendous flow of current in the sea level. A Polar bear is a gigantic animal which damages all sorts of debris ahead of them while locomotion. It develops a separate entity inside the arctic region and survives for years together. No separate entity is to be developed around the globe outside arctic region. There is no denying the fact that the Polar Bears are dreadful animalsand as such hunting of polar bears is difficult. The smelling power of polar bear is very high for which it can easily learn the whereabouts of the prey. The hunter generally shoots from a long distant apart to the polar bear and suffice it to say, it is very cumbersome to reach them by haunting but it is tamed by long time technical training and observation thoroughly the nature of the animals.

Canada is homespun to circa 16 000 of the appraised 20 000–25 000 polar bears in the global polar areas. It is no wonder that the polar bear, an icon of Canada’s wildlife heritage, is of great cultural significance to the Canadian people. For the Inuit and many northern communities, polar bears are especially significant culturally, spiritually and economically. Canada has a solepreservationconcern to safeguard these iconic creatures. This is one reason why Canada has amplified investment in observing efforts in current years. Canada’s portfolio schedule for polar bears is designed to ensure that there are up-to-date population estimates for all 13 subpopulations that occur in our country. While monitoring is thought-provoking due to the distant and inhospitable environment of the Arctic, population estimates can help ensure that management and upkeep actions are applicable.

In view of the above, global warming is a great threat to the survival of the polar bears, a wide ranging dangerous species  throughout the world. In the field of ecological balances in between the living and the non-living things, polar bears play a vital role to keep our environment healthy and pollution free.

Oxidation-Reduction Reactions

Rules for Assigning Oxidation States

 

The oxidation state (OS) of an element corresponds to the number of electrons, e^-, that an atom loses, gains, or appears to use when joining with other atoms in compounds. In determining the OS of an atom, there are seven guidelines to follow:

1.       The OS of an individual atom is 0.

2.       The total OS of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge.

3.       Group 1 metals have an OS of +1 and Group 2 an OS of +2

4.       The OS of fluorine is -1 in compounds

5.       Hydrogen generally has an OS of +1 in compounds

6.       Oxygen generally has an OS of -2 in compounds

7.       In binary metal compounds, Group 17 elements have an OS of -1, Group 16 of -2, and Group 15 of -3.

(Note: The sum of the OSs is equal to zero for neutral compounds and equal to the charge for polyatomic ion species.)

le 1: Assigning OSs

Determine the OSs of the elements in the following reactions: a.        Fe(s)+O2(g)→Fe2O3(g) b.       Fe2+ c.        Ag(s)+H2S→Ag2S(g)+H2(g) SOLUTIONS A.       Fe and O2 are free elements; therefore, they each have an OS of 0 according to Rule #1. The product has a total OS equal to 0, B.        and following Rule #6, O has an OS of -2, which means Fe has an OS of +3. C.       The OS of Fe corresponds to its charge; therefore, the OS is +2. D.      Ag has an OS of 0, H has an OS of +1 according to Rule #5, S has an OS of -2 according to Rule #7, and hence Ag in Ag2S has an OS of +1.

Example 2: Assigni

Determine the OS of the bold element in each of the following: A.       Na3PO3 B.       H2PO4- SOLUTIONS A.       The oxidation numbers of Na and O are +1 and -2. Because sodium phosphite is neutral, the sum of B.         C.       the oxidation numbers must be zero. Letting x be the oxidation number of phosphorus, 0= 3(+1) + x + 3(-2). D.       x=oxidation number of P= +3.  E.       Hydrogen and oxygen have oxidation numbers of +1 and -2. The ion has a charge of -1, so the sum F.       of the oxidation numbers must be -1. Letting y be the oxidation number of phosphorus, -1= y + 2(+1) +4(-2), y= oxidation G.       number of P= +5.

Example 3: Identifying Reduced and Oxidized Elements

Determine which element is oxidized and which element is reduced in the following reactions (be sure to include the OS of each):  A.       Zn + 2H+ → Zn2+ + H2 B.       2Al + 3Cu2+→2Al3+ +3Cu C.       CO32- + 2H+→ CO2 + H2O SOLUTIONS A.       Zn is oxidized (Oxidation number: 0 → +2); H+ is reduced (Oxidation number: +1 → 0) B.       Al is oxidized (Oxidation number: 0 → +3); Cu2+ is reduced (+2 → 0) C.       This is not a redox reaction because each element has the same oxidation number in both reactants and products: D.       O= -2, H= +1, C= +4. (For further discussion, see the article on oxidation numbers).

An atom is oxidized if its oxidation number increases, the reducing agent, and an atom is reduced if its oxidation number decreases, the oxidizing agent. The atom that is oxidized is the reducing agent, and the atom that is reduced is the oxidizing agent. (Note: the oxidizing and reducing agents can be the same element or compound).

Oxidation-Reduction Reactions

Redox reactions are comprised of two parts, a reduced half and an oxidized half, that always occur together. The reduced half gains electrons and the oxidation number decreases, while the oxidized half loses electrons and the oxidation number increases. Simple ways to remember this include the mnemonic devices OIL RIG, meaning "oxidation is loss" and "reduction is gain," and LEO says GER, meaning "loss of e^- = oxidation" and "gain of e^- = reduced." There is no net change in the number of electrons in a redox reaction. Those given off in the oxidation half reaction are taken up by another species in the reduction half reaction.

The two species that exchange electrons in a redox reaction are given special names. The ion or molecule that accepts electrons is called the oxidizing agent; by accepting electrons it causes the oxidation of another species. Conversely, the species that donates electrons is called the reducing agent; when the reaction occurs, it reduces the other species. In other words, what is oxidized is the reducing agent and what is reduced is the oxidizing agent. (Note: the oxidizing and reducing agents can be the same element or compound, as in disproportionate reactions).

A good example of a redox reaction is the thermite reaction, in which iron atoms in ferric oxide lose (or give up) O atoms to Al atoms, producing Al₂O₃.

Fe2O3(s)+2Al(s)→Al2O3(s)+2Fe(l)

Another example of the redox reaction is the reaction between zinc and copper sulfate.

Example 4: Identifying Oxidized Elements

Using the equations from the previous examples, determine what is oxidized in the following reaction. Zn+2H+→Zn2++H2 SOLUTION The OS of H changes from +1 to 0, and the OS of Zn changes from 0 to +2. Hence, Zn is oxidized and acts as the reducing agent.

Example 5: Identifying Reduced Elements

What is reduced species in this reaction? Zn+​2H+→Zn2++H2 SOLUTION The OS of H changes from +1 to 0, and the OS of Zn changes from 0 to +2. Hence, H+ ion is reduced and acts as the oxidizing agent.

Combination Reactions

Combination reactions are among the simplest redox reactions and, as the name suggests, involves "combining" elements to form a chemical compound. As usual, oxidation and reduction occur together. The general equation for a combination reaction is given below:

A+B→AB

Example 6: Combination Reaction

Equation: H2 + O2 →H2O Calculation: 0 + 0 → (2)(+1) + (-2) = 0 Explanation: In this equation both H2 and O2 are free elements; following Rule #1, their OSs are 0. The product is H2O, which has a total OS of 0. According to Rule #6, the OS of oxygen is usually -2. Therefore, the OS of H in H2O must be +1.

Decomposition Reactions

A decomposition reaction is the reverse of a combination reaction, the breakdown of a chemical compound into individual elements:

AB→A+B

Example 7: Decomposition Reaction

Consider the decomposition of water: H2O→H2+O2 Calculation: (2)(+1) + (-2) = 0 → 0 + 0 Explanation: In this reaction, water is "decomposed" into hydrogen and oxygen. As in the previous example the  H2O has a total OS of 0; thus, according to Rule #6 the OS of oxygen is usually -2, so the OS of hydrogen in H2O must be +1.

Single Replacement Reactions

A single replacement reaction involves the "replacing" of an element in the reactants with another element in the products:

A+BC→AB+C

Example 8: Single Replacement Reaction

Equation: Cl2+NaBr−−−→NaCl−−+Br2 Calculation: (0) + ((+1) + (-1) = 0) -> ((+1) + (-1) = 0) + 0 Explanation: In this equation, Br is replaced with Cl, and the Cl atoms in Cl2 are reduced, while the Br ion in NaBr is oxidized.

Double Replacement Reactions

A double replacement reaction is similar to a double replacement reaction, but involves "replacing" two elements in the reactants, with two in the products:

AB+CD→AD+CB

Example 9: Double Replacement Reaction

Equation: Fe2O3 + HCl → FeCl3 + H2O Explanation: In this equation, Fe and H trade places, and oxygen and chlorine trade places.

Combustion Reactions

Combustion reactions almost always involve oxygen in the form of O₂, and are almost always exothermic, meaning they produce heat. Chemical reactions that give off light and heat and light are colloquially referred to as "burning."

CxHy+O2→CO2+H2O

Although combustion reactions typically involve redox reactions with a chemical being oxidized by oxygen, many chemicals "burn" in other environments. For example, both titanium and magnesium burn in nitrogen as well:

2Ti(s)+N2(g)→2TiN(s)

3Mg(s)+N2(g)→Mg3N2(s)

Moreover, chemicals can be oxidized by other chemicals than oxygen, such as Cl₂ or F₂; these processes are also considered combustion reactions

Disproportionate Reactions

Disproportionate Reactions: In some redox reactions a single substance can be both oxidized and reduced. These are known as disproportionation reactions, with the following general equation:

2A→A+n+A−n

Where n is the number of electrons transferred. Disproportionate reactions do not need begin with neutral molecules, and can involve more than two species with differing oxidation states (but rarely).

Disproportionate reactions have some practical significance in everyday life, including the reaction of hydrogen peroxide,  H2O2 poured over a cut. This a decomposition reaction of hydrogen peroxide, which produces oxygen and water . Oxygen is present in all parts of the chemical equation and as a result it is both oxidized and reduced. The reaction is as follows: 2H2O2(aq)→2H2O(l)+O2(g) Explanation: On the reactant side, H has an OS of +1 and O has an OS of -1, which changes to -2 for the product H2O (oxygen is reduced), and 0 in the product O2 (oxygen is oxidized).

Street Racing

My advertising campaign is about illegal street car racing everywhere around the world. I chose this campaign because this is one of the problems that are causing a lot of deaths from car crashes and a lot of street racers are gong to jail for racing. My message to all the street racers is to bring to a standstill doing unlawful street race.

I used a slogan to tell my message on my poster. My slogan is “Street + Racing = Death or Jail”. It means that whatever a street racer does, that person cannot escape to die from car crashes or going to jail by getting busted by the cops. So what’s the point of street racing, street racers can just stay in a normal life. I used an image of two street racers doing illegal street race on my poster. I made a bright red ban symbol on the image; I did it to illustrate the message to stop doing illegal street racing. I made the outlaw symbolizing colour bright red to show that it is causing death. This image is related to my slogan. I used an image of a very bad car crash on my poster to show how people can die from a car crash. I chose a bad car crash image to scare the street racers and showed them how painfully they can die. I wrote “=Death” beside the image. I used an image of a person going to jail to show the street racers that if they do street racing, they will go to jail. I wrote “=Jail” beside the image.

I used a wristband as my gimmick. It is a very simple white wristband. On the wristband, I stacked my slogan on it. The wristband will cost $5. I will sell my band all across the world to spread my message everywhere. I will use 50% of the money that I earn to give it to the government to make new rules to stop illegal street racing. I came up with this idea because I saw people selling wristbands in the market and the money that the company of the wristbands earns uses some of the earnings for charity. So I thought my one could be sold like this.

My event is a concert to ban illegal street racing. I will organize a concert because many people in the world are interested in concerts and it is a good way to advertise my gimmick. I will also use some of the money that I earn to give to the government to make new rules to stop illegal street racing. I will call Linkin Park and Pod to play their rock bands. In the concert one of the members from the rock bands will tell everyone the message I am saying to everyone using my slogan and about my gimmick. I will show the concert in MTV channel so that the people that are not going to the concert know about my gimmick and my message. I came up with this idea because I saw many people organizing concerts and they use some of the money that they earn for charity. So I thought I could organize a concert and use the money like this.

In view of the above, it is evident that, for my campaign, I tried to make people aware of illegal street racing that is going on around the world. The visual techniques of advertising I used were juxtaposition, balance, background, font, colour, contrast and dominant image. I only used slogan as one of my language techniques of advertising. I hope I can make illegal street racers be aware of street racing by showing my poster, event and gimmick.