Using to
compare: the elements
The
periodic system is the periodic table illustrating a layout state, period and
type of chemical elements, periodic system is based on the increase in the
number Atom (increase the number of protons or nuclear charge). The periodic
system is divided into periods of the elements located in horizontal rows and
groups, namely the elements located in the vertical column.
1. Group
and Period of the Elements in the Periodic Table
The elements located on an upright column called groups. The classes are
numbered I, II, III, and so on. For example, Group II consists of the elements
beryllium, magnesium, and calcium.
The elements in horizontal rows called periods. For example, eight elements
ranging sodium to argon is located in one period. These elements have the same
pattern of the electron structure. Of lithium to neon, the number of electrons
in the outer shell increases from period 1 to 8. Then repeat again in the next
period of the sodium in the period 1 to argon in the period 8. In each group,
the number of electrons in the outer shell of each element is always the same in
accordance with the number class. For example, fluorine and chlorine both are
elements in Groups VII, the two elements have seven electrons in the outer
shell. The electronic structure is very important to understand the properties
of elements on the Periodic Table System.
2. Nature
of the Periodic Elements
What is meant by the periodic nature is that there is a relationship between
the properties of an element with its location on the Periodic Table System.
These properties are changed and repeated periodically, in accordance with
changes in the atomic number and electron configuration.
a. Atomic
radius
Atomic radius is the distance from the nucleus to the electrons in the outer
shell. Also known as the radius of positive ions and negative ionic radii. For
the elements of a class: Atomic radius greater the further down. Because of the
amount of skin that held the atoms more, then the outer shell farther from the
nucleus. To the elements during the same: Atomic radius shorter than left to
right. Though the number of shared skin, but the number of protons increases so
that the outermost electrons pulled closer towards the core.
The
radius of positive ions:
If an
atom loses electrons to form positive ions (cations),
X → X + +
e
Cation number more protons than electrons. These cations radii smaller than the
radius of the atom. This is due to the release of the outer electrons resulting
in the skin is reduced.
The
radius of negative ions:
If an
atom captures electrons to form negative ions (anions),
Y + e → Y
In the anion amount more electrons than protons. This anion radii larger than
the radius of the atom. Because of this extra electron results in the skin
increases.
b. The
ionization energy
The ionization energy is the minimum energy required to remove the outermost
electron from an atom in the gas state. In general concluded that:
• The
greater the ionization energy, the more difficult it is to release the outer
electrons of atoms. So the more stable the atom.
• The
ionization energy of the elements in one class from top to bottom on the wane
• The
ionization energy of the elements in a period from left to right are
increasingly getting bigger.
c.
Electron affinity
Electron affinity is the energy released in the form of an atom when it
receives an electron gas. There are still many atoms are not known electron
affinity prices, because pricing direct electron affinities difficult.
In
general concluded that:
• The
larger the electron affinity of an atom price, the easier these elements form a
negative ion.
•
electron affinity of the elements in one class from top to bottom on the wane.
•
Electron affinity elements in a period of growing left to right.
d.
Electronegativities
Electronegativity is a measure of the ability of an atom to attract electrons
in the bond. The magnitude of the price relative electronegativity between an
atom to another atom. In the periodic table it can be concluded:
•
Elements in one class from top to bottom on the wane.
•
Elements in a period of greater left to right.
e. The
nature of the metal element
The arrangement of the elements in the periodic system are also grouped into
metals and non-metals. The boundary between the metal and nonmetal is not so
clear because there are some elements that can have properties of metals and
non-metals, these elements include semi-metal or metalloid group. Metalloid
elements located on the boundary line of a diagonal ladder, namely B, Si, Ge,
As, Sb and Te. The left boundary line laid metal elements, non-metallic
elements being located on the right.
In the
periodic table it can be concluded:
• In one
class from top to bottom metal properties increased.
• In the
period from left to right on the wane metal properties
f.
Reactivity
Reactive means easy to react. Metallic elements in the periodic system, more
and more reactive to the bottom, because more easily release electrons.
Non-metal elements in the periodic system, further down, the less reactive,
because more and more difficult to capture electrons.
Reactivity of an element depends on the inclination release or pull electrons.
Thus, the most reactive metals are group VIIA (halogen). From left to right in
a period, initially decreased reactivity was increased to group VIIA. Group
VIIA unreactive.
Elements
of Metal
Metal is
the element that has the shiny properties and generally conduct electricity and
a good conductor of heat. Metal elements are generally solid at normal
temperature and pressure, except for mercury in liquid form. In general,
malleable metallic element that can be formed into other objects.
Non
Metallic Elements
The
non-metallic element is an element that does not have metal-like properties. In
general, non-metallic elements are gaseous and solid at normal temperature and
pressure. Examples of non-metallic elements which are gaseous oxygen, nitrogen,
and helium. Examples of non-metals that are solid are sulfur, carbon,
phosphorus, and iodine. The non-metallic solids are usually hard and brittle.
The non-metallic element that is a liquid is bromine.
Elements
Semi Metal
In
addition to metal and nonmetal elements there are also elements semilogam or
known as metalloid. Metalloid is an element that has the properties of metals
and non-metals. Semilogam element is usually a semiconductor. What is a
semiconductor? Semiconductor material which is not able to conduct electricity
well at low temperatures, but the nature of the electrical conductivity becomes
better when the temperature is higher.
Source:
https://rahmikimia.wordpress.com/kimia-kelas-x/2-sistem-periodik-unsur/c-sifat-sistem-periodik/
http://webcache.googleusercontent.com/search?q=cache:sdZcQN43ANAJ:tri_surawan.staff.gunadarma.ac.id/Downloads/files/40823/Bab9_TabelPeriodik_A4.pdf+&cd=11&hl=id&ct=clnk&gl=id
Do neutrons bind to electrons? If not why?
BalasHapusNeutrons or neutrons are subatomic particles that are neutral and have a mass of 940 MeV / c² (1.6749 × 10-27 kg, slightly heavier than protons.) The rotation is ½.
HapusThe atomic nucleus of most atoms (all except the most common Hydrogen isotope, consisting of a proton) consists of protons and neutrons.
Outside the atomic nucleus, the neutron is unstable and has a half-life of about 15 minutes (881.5 ± 1.5 seconds), melts by emitting electrons and antineutrino to become protons. The same decay method (beta decay) occurs in some nuclei. The particles in the atomic nucleus are usually neutrons and protons, which are transformed into one and the other by the transmission and absorption of the pawn. A neutron is classified as a baryon and consists of two bottom quarks and one upper quark. The neutron equation of the antibody is antineutron.
The main difference between neutrons and other subatomic particles is that they are not charged. This neutral nature makes its discovery more backward, and deeply penetrating, making it difficult to observe directly and making it extremely pentin as an agent in nuclear change.
Rutherford's research in addition to the success of getting some satisfactory results also get an awkwardness ie the atomic nucleus mass of an element is always greater than the mass of protons in the nucleus of the atom. Rutherford suspects that there are other particles in the nucleus that are uncharged because the atoms are positively charged because of the positively charged protons. The presence of other particles in the uncharged nucleus of atoms was evidenced by James Chadwick in 1932. Chadwick conducted research by shooting beryllium metal using alpha rays. The results show that an uncharged particle is released when beryllium metal is shot with alpha rays and these particles are called neutrons.
Electrons are subatomic particles that are negatively charged and are generally written as e-. Electrons have no known underlying components or substructures, so they are believed to be elementary particles. Electrons have a mass of about 1/1836 mass of protons. The intrinsic angular momentum (spin) of electrons is half the integer value in units ħ, which means that it includes fermions. Electron antiparticles are called positrons, which are identical to electrons, but positively charged. When an electron collides with a positron, both are likely to split into one another or destroy completely, producing a pair (or more) gamma ray photons.
The electrons, which belong to the family generation of the first lepton particles, participate in gravitational interactions, electromagnetic interactions and weak interactions. Like all matter, electrons have both particle and wave-like properties (wave-particle duality), so they can collide with other particles and diffract like light. Since electrons include fermions, two different electrons can not occupy the same quantum state according to the Pauli exclusion principle.
The concept of an undivided electrical charge was theorized to explain the chemical properties of atoms by the natural philosopher Richard Laming in early 1838; The name electron was introduced to name this charge in 1894 by Irish physicist George Johnstone Stoney. Electrons were identified as particles in 1897 by J. J. Thomson.
can u explain to me about Elements of Metal,Non Metallic Elements and Elements Semi Metal?
BalasHapusMetals are elements that have shiny properties and are generally good conductor of electricity and heat conductor. Metal elements are generally solid at normal temperatures and pressures, except for mercury in the form of liquid. In general, metal elements can be forged so that it can be formed into other objects.
HapusCharacter :
- Good electrical conductor
- Shiny
- Can be forged and stretched
- At room temperature in solid form except mercury
- Has high melting and boiling points
Examples of metal elements:
A. Group IA, except hydrogen
B. Group IIA
C. Group IIIA, except boron
D. Group IIIB-IIB
E. Group IVA = lead and lead
F. Type VA = bismuth
The non-metallic element is an element which has no metallic properties. In general, non-metallic elements are gaseous and solid at normal temperature and pressure. Examples of non-metallic elements in the form of gases are oxygen, nitrogen, and helium. Examples of non-metallic elements in solid form are sulfur, carbon, phosphorus, and iodine. Non-metallic solids are usually hard and brittle. Non-metallic element in the form of liquid is bromine.
Character :
- Electrical insulator
- Not shiny
- Usually ruptured if forged and can not be stretched
- At room temperature in the form of liquid and gas, but some are solid
- Has a low boiling point and melting point
Non-metallic element example:
A. Group IA = hydrogen
B. Group IVA = carbon
C. Type VA = nitrogen, phosphorus
D. Group VIA = oxygen, sulfur, selenium
E. Group VIIA = Phosphorus, Clorin, Bromine, Iodine
F. Group VIII
In addition to metal and nonmetal elements there is also a semilogam element or known as a metaloid. Metaloid is an element that has metallic and nonmetal properties. Semilogam element is usually semiconductor. What is a semiconductor? Semiconductor materials can not conduct electricity well at low temperatures, but their electrical conductivity becomes better when the temperature is higher.
Properties: the transition between metal elements and nonmetallic elements.
Examples of semi-metallic elements:
A. Group IIIA = boron
B. Group IVA = silicon, germanium
C. Type VA = arsenic, antimony
D. Group VIA = tellurium, polonium
are you have a tips for compare or contrasting element ?
BalasHapuslike make a double buble maps or something thank you
First of all must master the material to be compared. Then proceed by comparing from the most basic to comparing to the higher level.
Hapuswhat are the caracteristic from elements, and which about differit from others
BalasHapusA material element consisting of one atom or more types which has the same thing compose a substance. The smallest particle of an element is an atom. element is the constituent material of a substance that has the same properties. Elements are distinguished by their atomic number (number of protons in their nucleus). Elements cannot be broken down into simpler substances by chemical reactions.
Hapus