Understanding
Atom
Atom is the smallest part of an element that still has the properties of that element. Each atom of an element have different properties to the atomic nature of the other elements.
Atom is the smallest part of an element that still has the properties of that element. Each atom of an element have different properties to the atomic nature of the other elements.
Development of Atomic Theory
- In 400 BC Democritus and Leucippus states that all matter is composed by particles are very small and can not be divided again. And then they named the atom with greek (atomos: a = no, Tomos = cut or split). Whereas Aristotle states that matter is continuous, meaning that the material can be split or shared continuously without limit.
- In 1803 John Dalton (1766-1844) Atomic Model Dalton à states:
· The material is composed of small particles tidakdapat divided again,
· Atoms of the same (an element) has the same properties
· Atoms can join together chemically to form moleku
Weaknesses: does not explain the difference between atomic elements with other atoms
- In 1898 JJ Thomson (1856-1940) stated à Thomson Atomic Model:
· Atomic incandescent spherical positively charged and contains a number of electrons in the negatively charged atoms
· The number of positive and negative charges the same, so the charge is neutral atoms
- In 1911 Ernest Rutherford (1887-1931) Model àmenyatakan Rutherford:
· Atomic nucleus contains positively charged atom in the center and surrounded by negatively charged electrons
Weakness: not able to explain why the electrons do not fall into the nucleus due to the gravity of the core electrons
- Niels Bohr Model à states
· Electrons can spin only through a particular trajectory
· If the electron perpindah kelintasan deeper, it will be emitted energy whereas when you go out it will be absorbed energy
Weaknesses: can not explain the spectrum of colors from many electron atoms.
- Erwin Schrodinger and Warner Heisenbreg (1925-1926) stated à-Heisenbreg Schrodinger Atomic Model: electrons can be determined only possible where it is, which is located in a space called the electron cloud.
- In 400 BC Democritus and Leucippus states that all matter is composed by particles are very small and can not be divided again. And then they named the atom with greek (atomos: a = no, Tomos = cut or split). Whereas Aristotle states that matter is continuous, meaning that the material can be split or shared continuously without limit.
- In 1803 John Dalton (1766-1844) Atomic Model Dalton à states:
· The material is composed of small particles tidakdapat divided again,
· Atoms of the same (an element) has the same properties
· Atoms can join together chemically to form moleku
Weaknesses: does not explain the difference between atomic elements with other atoms
- In 1898 JJ Thomson (1856-1940) stated à Thomson Atomic Model:
· Atomic incandescent spherical positively charged and contains a number of electrons in the negatively charged atoms
· The number of positive and negative charges the same, so the charge is neutral atoms
- In 1911 Ernest Rutherford (1887-1931) Model àmenyatakan Rutherford:
· Atomic nucleus contains positively charged atom in the center and surrounded by negatively charged electrons
Weakness: not able to explain why the electrons do not fall into the nucleus due to the gravity of the core electrons
- Niels Bohr Model à states
· Electrons can spin only through a particular trajectory
· If the electron perpindah kelintasan deeper, it will be emitted energy whereas when you go out it will be absorbed energy
Weaknesses: can not explain the spectrum of colors from many electron atoms.
- Erwin Schrodinger and Warner Heisenbreg (1925-1926) stated à-Heisenbreg Schrodinger Atomic Model: electrons can be determined only possible where it is, which is located in a space called the electron cloud.
Atomic Structure
Ø atomic model that can be used to study the atomic structure is Rutherford and Bohr model of the atom.
Ø Bohr's atomic model is similar to the position of the sun to the planets in the solar system. The mass of the nucleus is much larger than the electron mass. Therefore, the electrons surrounding the nucleus.
- Atoms consist of a nucleus and electrons. The nucleus is composed of protons and neutrons.
- Protons are positively charged (+), uncharged neutrons (neutral), while the electrons are negatively charged (-). Same number of electrons and protons, so the atom becomes neutral charge.
- The number of protons and electrons are expressed as atomic number, number of protons and neutrons is expressed as the mass of the atom. Arrangement of atoms can be written using the following notations:
Rounded Rectangle: (_ ^ A) X_z ^ Description:
X = symbol element
A = atomic mass = number of protons + number of neutrons
Z = atomic number = number of protons = number of electrons
A-Z = Number of neutrons
Ø atomic model that can be used to study the atomic structure is Rutherford and Bohr model of the atom.
Ø Bohr's atomic model is similar to the position of the sun to the planets in the solar system. The mass of the nucleus is much larger than the electron mass. Therefore, the electrons surrounding the nucleus.
- Atoms consist of a nucleus and electrons. The nucleus is composed of protons and neutrons.
- Protons are positively charged (+), uncharged neutrons (neutral), while the electrons are negatively charged (-). Same number of electrons and protons, so the atom becomes neutral charge.
- The number of protons and electrons are expressed as atomic number, number of protons and neutrons is expressed as the mass of the atom. Arrangement of atoms can be written using the following notations:
Rounded Rectangle: (_ ^ A) X_z ^ Description:
X = symbol element
A = atomic mass = number of protons + number of neutrons
Z = atomic number = number of protons = number of electrons
A-Z = Number of neutrons
Electron Configuration
- Electrons surround the nucleus of an atom on the trajectories (shells) with a certain energy level. The arrangement of electrons in an atom is called the electron configuration shell.
- The number of electrons that can be accommodated masimum each skin is 2N2 where n is the number of skin. For the first 20 elements of the outer shell is not more than 8 electrons, for example, potassium has 19 electrons and its configuration is not 2 8 8 1 2 8 9.
Ø Ion
ü Ions are electrically charged particles that are formed when an atom loses an electron or or more to form a stable outer shell. Ion that lost an electron positively charged (cations) and the capture of an electron is negatively charged (anionic).
ü event release or influx of ions is called ionization. Ion was first discovered by the German physicist, Julius Elster and Hans Friedrich Geitel in 1899.
ü Proton is located in the nucleus of an atom that prtoton hard to get out of the atom. To remove the proton required enormous energy (nuclear reaction). Electrons are outside the nucleus (around the nucleus of an atom in a particular orbit) so that the electrons can leave a an atom. Furthermore, the electron is accepted by the other atom. In other words, an atom can release or accept electrons.
- Electrons surround the nucleus of an atom on the trajectories (shells) with a certain energy level. The arrangement of electrons in an atom is called the electron configuration shell.
- The number of electrons that can be accommodated masimum each skin is 2N2 where n is the number of skin. For the first 20 elements of the outer shell is not more than 8 electrons, for example, potassium has 19 electrons and its configuration is not 2 8 8 1 2 8 9.
Ø Ion
ü Ions are electrically charged particles that are formed when an atom loses an electron or or more to form a stable outer shell. Ion that lost an electron positively charged (cations) and the capture of an electron is negatively charged (anionic).
ü event release or influx of ions is called ionization. Ion was first discovered by the German physicist, Julius Elster and Hans Friedrich Geitel in 1899.
ü Proton is located in the nucleus of an atom that prtoton hard to get out of the atom. To remove the proton required enormous energy (nuclear reaction). Electrons are outside the nucleus (around the nucleus of an atom in a particular orbit) so that the electrons can leave a an atom. Furthermore, the electron is accepted by the other atom. In other words, an atom can release or accept electrons.
The valence electrons:
- Establishment of positive ions à atom loses electrons
- The formation of negative ions capture electrons à atom
- Ionikàsenyawa compound formed from positive ions and negative ions bond together to form a neutral compound. Ionic compounds have a high melting point. That's because the compound there is a very strong bond between the ions forming
Ø Molecular
ü The molecule is the smallest part of a compound and still have the properties of these compounds. In other words, the molecule is a combination of two or more atoms chemically.
ü Based on the types of atoms that make up molecules, molecules are divided into two, namely:
- Molecular Elements à bunch of atoms of the same element chemically combine to form a molecule. In other words, the molecule consists of only one type of constituent atoms.
The molecule can be divided into two elements, namely:
· Molecular diatomikàmolekul element composed of two atoms of the same. Example: H2 (hydrogen), O2 (oxygen gas)
· Molecular poliatomikà molecular elements composed of more than two of the same atom. Example: P4, S8
Examples of elements of hydrogen formation
ü Each hydrogen atom has satuelektron
ü electrons are trying to form a stable electron configuration, ie two (the maximum number of electrons on the skin to-1)
ü The two electrons have enough power to attract each other
ü The atoms used by two atoms (sharing)
ü Each nucleus has two electrons in the atomic shell.
Covalent bond
ü bonds are bonds that form due to the use of electrons together
ü Iakatan covalent ionic bond is less powerful than
ü If there is 1 atom pairs are used together, it is called a single covalent bond
ü If there are 2 pairs of atoms that are used together, it is called a double covalent bond
ü The electrons are not shared are called nonbonding electrons (bonding = bond)
ü covalent Senayawa not conduct electricity because it does not form ions are electrically charged.
- Molecular compounds à compounds composed of more than one type of constituent atoms.
Example: H2O (water), CO2 (carbon dioxide)
Examples formation of water molecules
ü The water molecule consists of two atoms of H and 1 atom O
ü Atomic H has 1 electron in its outer shell
ü Atom O has 6 electrons in its outer shell
ü Each H atom to one electron eletron by pulling 2 of 2 atoms O
ü Atom O requires two atoms. The trick is to draw two electrons of two atoms H
ü There are two covalent bonds.
Ø Atoms, Ions, Molecules in Daily Chemical Products
ü Breathing a breath of air molecules udaramengandung elements such as oxygen (O2), nitrogen (N2), and the molecules of compounds such as carbon dioxide (CO2) emissions.
ü The sweetness of sugar molecules composed of sugar or sucrose (C12H22O11).
ü taste sour pickles, a few drops of vinegar derived from molecules containing vinegar (CH3COOH).
ü kitchen salt derived from a chemical compound that is NaCl, which if dilarut in water into ions Na + and Cl-
ü Gasoline or diesel fuel composed of hydrocarbon molecules
ü Glass, glasses, plates consist of molecules of silica oxide (SiO2)
ü plastic polymers include polyethylene, polypropylene, polyurethane, and PVC
ü polymer is polyisoprene rubber and polystyrene.
- Establishment of positive ions à atom loses electrons
- The formation of negative ions capture electrons à atom
- Ionikàsenyawa compound formed from positive ions and negative ions bond together to form a neutral compound. Ionic compounds have a high melting point. That's because the compound there is a very strong bond between the ions forming
Ø Molecular
ü The molecule is the smallest part of a compound and still have the properties of these compounds. In other words, the molecule is a combination of two or more atoms chemically.
ü Based on the types of atoms that make up molecules, molecules are divided into two, namely:
- Molecular Elements à bunch of atoms of the same element chemically combine to form a molecule. In other words, the molecule consists of only one type of constituent atoms.
The molecule can be divided into two elements, namely:
· Molecular diatomikàmolekul element composed of two atoms of the same. Example: H2 (hydrogen), O2 (oxygen gas)
· Molecular poliatomikà molecular elements composed of more than two of the same atom. Example: P4, S8
Examples of elements of hydrogen formation
ü Each hydrogen atom has satuelektron
ü electrons are trying to form a stable electron configuration, ie two (the maximum number of electrons on the skin to-1)
ü The two electrons have enough power to attract each other
ü The atoms used by two atoms (sharing)
ü Each nucleus has two electrons in the atomic shell.
Covalent bond
ü bonds are bonds that form due to the use of electrons together
ü Iakatan covalent ionic bond is less powerful than
ü If there is 1 atom pairs are used together, it is called a single covalent bond
ü If there are 2 pairs of atoms that are used together, it is called a double covalent bond
ü The electrons are not shared are called nonbonding electrons (bonding = bond)
ü covalent Senayawa not conduct electricity because it does not form ions are electrically charged.
- Molecular compounds à compounds composed of more than one type of constituent atoms.
Example: H2O (water), CO2 (carbon dioxide)
Examples formation of water molecules
ü The water molecule consists of two atoms of H and 1 atom O
ü Atomic H has 1 electron in its outer shell
ü Atom O has 6 electrons in its outer shell
ü Each H atom to one electron eletron by pulling 2 of 2 atoms O
ü Atom O requires two atoms. The trick is to draw two electrons of two atoms H
ü There are two covalent bonds.
Ø Atoms, Ions, Molecules in Daily Chemical Products
ü Breathing a breath of air molecules udaramengandung elements such as oxygen (O2), nitrogen (N2), and the molecules of compounds such as carbon dioxide (CO2) emissions.
ü The sweetness of sugar molecules composed of sugar or sucrose (C12H22O11).
ü taste sour pickles, a few drops of vinegar derived from molecules containing vinegar (CH3COOH).
ü kitchen salt derived from a chemical compound that is NaCl, which if dilarut in water into ions Na + and Cl-
ü Gasoline or diesel fuel composed of hydrocarbon molecules
ü Glass, glasses, plates consist of molecules of silica oxide (SiO2)
ü plastic polymers include polyethylene, polypropylene, polyurethane, and PVC
ü polymer is polyisoprene rubber and polystyrene.
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