using english to compare : the elements

COMPARE AND CONTRAST

(SAME AND DIFFERENCE

1.  Compare

compare is looking for similarities between two or more of a case. in chemistry usually compared to the equation is that there are elements In nature both metallic and non-metallic. examples of calcium and magnesium equation

CALCIUM

MAGNESIUM

2. Contrast

contrast is also a comparison between two or more of a case. 

were compared in contrast is the difference.

for example, the difference between the chemical elements such as potassium and strontium.

potassium

     strontium

NATURE OF PERIODIC ELEMENTS

1. ATOM FINGERS

The image in this bawwah shows the data of atomic radius. The radius of the atom is the distance of the outer electron to the nucleus of the atom and shows the size of an atom. The radius of the atom is difficult to measure so that the measurements of the radius of the atom are done by measuring the distance between the two nuclei of each other's bonded atom. In one class, the radius of the atoms increasingly upward tend to be smaller. This happens because the more up, the smaller the electron shell. In one period, the right to the radius of the atom tends to be smaller. This happens because the more to the right the number of protons and the number of electrons increases while the number of outer shells filled with electrons remains the same so that the pull of the nucleus to the electrons is stronger.

2. KEELEKTRONEGATIFAN

Electronegativity is the tendency of an atom to attract electrons. The relative price of electrogens is relative (a price comparison of an atom to another atom). One definition of electronegativity is Pauling's definition of quantitative-scale data. The trend of electronegative values ​​of elements In one class, the price of electronegativity from the bottom up is greater. In one period, from left to right the greater the price of electronegativity. The price of the electronegativity is important to determine the oxidation number (oxidation) of the element in a compound. If the price of electronegativity is large, the corresponding elements tend to accept electrons and form a negative oxidation number. If the price of electronegativity is small, the cenderun element releases the electrons and forms a positive oxidation number. The number of bonded atoms depends on the valence electrons (to be discussed in the chemical bond section). Thus the periodic nature of the element, the electronegativity is a number that describes the relative tendency of an element to attract an electron to its side in a chemical bond.

3. ENERGY IONIZATION (EI)

The ionisation energy is the minimum energy required of the neutral atom in the form of a gas to release an outer (weakest attached) electron to form a positive ion. The release of the second electron (from the positive ion one) is called the second ionisation energy, the release of a third electron is called the third ionization energy, and so on. Stages of electron discharges can be described as follows:

M (g) → M + (g) + e- Ei-1

M + (g) → M2 + (g) + e- Ei-2

The price of ionisation energy is affected by the radius of the atom and the number of valence electrons or nuclear charge. The smaller the radius of the atom, the price of ionization energy will be greater. The larger the nuclear charge, the energy of the ions will tend to increase.

4. ELECTRONIC AFITITY

Electron affinity is the energy liberated by one atom in the form of a gas when it receives an electron. The price of electron affinity is difficult to determine directly.

5. METAL AND NONLOGAM PROPERTIES

Chemically, metallic properties are associated with electropositive, ie the tendency of atoms to release electrons to form positive ions. Thus, the properties of the metal will depend on the ionization energy. The greater the ionisation energy, to release the electrons, and the less the metal properties. In contrast, non-metallic properties are associated with electronegativity, ie the tendency of atoms to attract electrons. In accordance with the tendency of ionization and electronegativity energy discussed above, the metallic and nonmetal properties in the periodic system of elements are as follows:

1. From left to right in a period, the metal properties decreases, while its non-metamic properties increase.

2. From top to bottom in one class, the nature of the metal increases, while the non-metallic properties decreases.

Thus, the metal element lies in the lower-left part of the periodic system of elements, while the non-metallic element lies on the right-top. However, the most non-metamic is the VIIA group, not the VIIIA group. The element located in the middle, the element located in the boundary between the metal and non-metal, has a metal and non-metallic properties. These elements are called metalloids. Examples are boron and silicon.

6. KEREAKTIFAN (EASY TO APPLY)

The reactivity of an element depends on its tendency to release or attract electrons. Thus, the most reactive metal element is group IA (alkali metal), whereas the most reactive non-metal is the VIIA group (halogen). From left to right in one period, first the clarity decreases and then increases to the VIIA group. Group VIIIA is not reactive.

DOUBLE BUBLE MAPS
·         What are the similar and different qualities of these things?
·         What qualities of each thing correspond to one another? In what way? 
·         Thinking process:
ü  This map is useful in comparing and contrasting two
ü  things. It allows for qualities that are shared to be placed in
ü  between the two items while differences are placed on the
ü  outside of the items.
ü  Unlike the bubble map, the words in the circles do not
ü  need to be limited to adjectives. You may use any words or
ü  phrases that are appropriate.
ü  Color coding the similarities/differences may make the
ü  relationships more obvious to see.
·         How to create this map:
ü  Near the center of your work space write the names of the two things that are being described. 
Each item should be in its own circle with space between the circles for details.
ü  In the middle of the two things being compared, write the common qualities.
 Each quality should have its own circle and 
should be connected with a line to the original item circles.
ü  On the outside of each original circle, 
you should write descriptions that are unique to each item.
 Every idea should each have its own circle and should only be connected with
 a line to what it describes.
Aurum (GOLD ) vs Argentum ( SILVER )

Comparebetween Gold and Silver are :







ü  Gold same like Silver they both are Metal


ü  We know they are element of group transitoin


ü  They are shining


ü  Gold same like Silver they are jewellery


ü  Gold as solid as Silver






















Contrastbetween Gold and Silver are :







ü  The Gold colour contras with The Silver colour.



 Because the colour of  aurum gold while the argentums silver


ü  argentums  is not aslimited as aurum


ü  aurum  more heavy than argentum



ü  The atomic number of aurum  higher than argentum



ü  aurum  more expensive than argentum