Acid - Acids are
compounds with a pH less than 7 that form hydrogen ions when dissolved in
water. Acids
react when in contact with bases and some metals to form salts.
Alkali metal - Alkali metal is an element in the first column of the periodic table with the exception of hydrogen.
Alkaline earth metal - Alkaline earth metal is an element in the second column of the periodic table.
Allotropes - Allotropes are different shapes in which the same element can exist. For example, carbon elements can be either allotropes of graphite or allotropes of diamonds.
Atoms - the atom is the fundamental unit of matter and the smallest unit of an element. It consists of a core surrounded by a cloud of electrons.
Bases - are substances with a pH higher than seven. A base is defined as a contributor to a pair of valence electrons.
Biochemistry - The study of chemical processes related to living organisms.
Loads - The attraction between the atoms that make up the chemicals.
Bunsen burner - A piece of chemical laboratory equipment that produces a fire used for laboratory experiments.
Carbon Cycle - A method by which carbon keeps moving throughout the biosphere.
Catalyst - A substance that accelerates the rate of a chemical reaction. The catalyst is not consumed in the reaction.
Chemical reactions - A process in which a set of substances undergoes chemical changes to form different substances.
Compounds - A chemical compound is a pure substance consisting of two or more elements.
Conductor - A conductor is a material that enables the flow of energy such as heat or electricity.
Covalent bonds - covalent bonds occur between atoms that share a pair of electrons to obtain their full outer shell.
Density - Density is mass per unit volume of substance. [Adsense]
Distillation - The process of separating the mixture by boiling the liquid and then recovering the cooled gas.
Elastic - Ability of material that will extend to long wire.
Electrolysis - A process used to drive a chemical reaction using an electric current. It is often used for separate elements.
Electrons - An atomic particles orbiting an atomic nucleus and carrying a negative charge.
Element - A pure chemical compound consisting of one type of atom. Every atom in an element is determined by the atomic number which is the number of protons in the nucleus.
Ions - An atom or molecule that has a negative or positive charge because the number of electrons is not equal to the number of protons.
Ionic bonds - ionic bonds are when an electron is exchanged between atoms to have a full outer shell.
Isotopes - Isotopes are atoms of the same element that have different amounts of neutrons.
Malleable - A substance is said to be soft if it can be ground into thin sheets.
Metals - A substance that is a conductor of heat and electricity. They are generally soft, elastic, and shiny.
Mixtures - Combinations of two or more chemically incorporated substances.
Molecules - Molecules are formed when two or more atoms are joined together by chemical bonds.
Neutrons - A particle in an atom's nucleus that has no electric charge.
The noble gas - A family of elements that make up the 18th column of the periodic table. They are very stable because the outer shell of the electrons is full.
Core - The nucleus is the center of the atom containing protons and neutrons.
Oxidation - The name for the process when oxygen combines with other elements to form compounds.
Periodic Table - A table of chemical elements arranged by atomic number.
The PH - pH scale measures the activity of hydrogen ions in a substance. If a substance has a pH less than 7 is said to be acidic. If the pH is greater than 7 then it is said to be alkaline or alkali.
Proton - A particle in a nucleus that holds a positive charge.
Reactions - Processes that occur when two or more chemicals are combined to form other chemicals.
Salt - Salt is a chemical compound formed by the reaction of acids and bases.
Solution - A homogeneous mixture is where a substance called a solute is completely dissolved into another substance called a solvent. For example, a solution is formed when a salt dissolves in water to make a brine solution.
Valence electrons - An electron in an atom that can participate in chemical bonds.
Amphoteric - The properties of a molecule that can behave as an acid that can donate protons on a strong base, or may also behave as a base that can accept protons from strong acids
Alkali metal - Alkali metal is an element in the first column of the periodic table with the exception of hydrogen.
Alkaline earth metal - Alkaline earth metal is an element in the second column of the periodic table.
Allotropes - Allotropes are different shapes in which the same element can exist. For example, carbon elements can be either allotropes of graphite or allotropes of diamonds.
Atoms - the atom is the fundamental unit of matter and the smallest unit of an element. It consists of a core surrounded by a cloud of electrons.
Bases - are substances with a pH higher than seven. A base is defined as a contributor to a pair of valence electrons.
Biochemistry - The study of chemical processes related to living organisms.
Loads - The attraction between the atoms that make up the chemicals.
Bunsen burner - A piece of chemical laboratory equipment that produces a fire used for laboratory experiments.
Carbon Cycle - A method by which carbon keeps moving throughout the biosphere.
Catalyst - A substance that accelerates the rate of a chemical reaction. The catalyst is not consumed in the reaction.
Chemical reactions - A process in which a set of substances undergoes chemical changes to form different substances.
Compounds - A chemical compound is a pure substance consisting of two or more elements.
Conductor - A conductor is a material that enables the flow of energy such as heat or electricity.
Covalent bonds - covalent bonds occur between atoms that share a pair of electrons to obtain their full outer shell.
Density - Density is mass per unit volume of substance. [Adsense]
Distillation - The process of separating the mixture by boiling the liquid and then recovering the cooled gas.
Elastic - Ability of material that will extend to long wire.
Electrolysis - A process used to drive a chemical reaction using an electric current. It is often used for separate elements.
Electrons - An atomic particles orbiting an atomic nucleus and carrying a negative charge.
Element - A pure chemical compound consisting of one type of atom. Every atom in an element is determined by the atomic number which is the number of protons in the nucleus.
Ions - An atom or molecule that has a negative or positive charge because the number of electrons is not equal to the number of protons.
Ionic bonds - ionic bonds are when an electron is exchanged between atoms to have a full outer shell.
Isotopes - Isotopes are atoms of the same element that have different amounts of neutrons.
Malleable - A substance is said to be soft if it can be ground into thin sheets.
Metals - A substance that is a conductor of heat and electricity. They are generally soft, elastic, and shiny.
Mixtures - Combinations of two or more chemically incorporated substances.
Molecules - Molecules are formed when two or more atoms are joined together by chemical bonds.
Neutrons - A particle in an atom's nucleus that has no electric charge.
The noble gas - A family of elements that make up the 18th column of the periodic table. They are very stable because the outer shell of the electrons is full.
Core - The nucleus is the center of the atom containing protons and neutrons.
Oxidation - The name for the process when oxygen combines with other elements to form compounds.
Periodic Table - A table of chemical elements arranged by atomic number.
The PH - pH scale measures the activity of hydrogen ions in a substance. If a substance has a pH less than 7 is said to be acidic. If the pH is greater than 7 then it is said to be alkaline or alkali.
Proton - A particle in a nucleus that holds a positive charge.
Reactions - Processes that occur when two or more chemicals are combined to form other chemicals.
Salt - Salt is a chemical compound formed by the reaction of acids and bases.
Solution - A homogeneous mixture is where a substance called a solute is completely dissolved into another substance called a solvent. For example, a solution is formed when a salt dissolves in water to make a brine solution.
Valence electrons - An electron in an atom that can participate in chemical bonds.
Amphoteric - The properties of a molecule that can behave as an acid that can donate protons on a strong base, or may also behave as a base that can accept protons from strong acids
Try to mention the example of the conductor ..
BalasHapusConductors are made of materials that electricity can flow through easily. These materials consist of atoms whose electrons can move freely.
HapusSome examples of conductors are:
Copper
Aluminum
Platinum
Gold
Silver
Water
People and Animals
Tree
Of the above vocabulary is about valence electrons, explain to me about it
BalasHapusValence electrons are the electrons of an atom that can form a chemical bond with other atoms. Valence electrons in a free neutral atom can bind to other valence electrons of other atoms to form chemical bonds.
HapusValence electrons can determine how the chemical features of the elements and whether they can bind to others or not.
Valence electrons have the ability, like electrons in deeper skin, to absorb or release energy in the form of photons. The absorption or discharge of energy can make an electron move (jump) to another skin or even apart from its atoms and valence shells.
Give me a biochemical reaction in daily life
BalasHapus1. Application of Biochemistry in the field of health
HapusWith the use of biochemistry in the field of health we can understand the health and choose our health to avoid the various diseases that exist. If we have been exposed to the disease we can also understand and do the handling of an illness effectively. In addition, Biochemistry can also explain things in the field of pharmacology and toxicology because these two fields are related to the influence of chemicals from outside to metabolism. Then in the case of Medicines usually affect certain metabolic pathways, for example penicillin antibiotics can kill bacteria by inhibiting the formation of polysaccharides in bacterial cell walls. Thus the bacteria will die because they can not form a cell wall.
2. Application of Biochemistry in agriculture
Some examples of the application of biochemistry in agriculture are in the process of using pesticides. In general, pesticides work by inhibiting enzymes that work on pests or certain organisms. In this case biochemistry plays a role in researching the pesticide's working mechanism so as to increase its selectivity and thus can be prevented from the negative environmental impact it can cause. In addition, improving the quality of products in agriculture and livestock can not be separated also from the role of biochemistry because with biochemistry we can realize and apply the results of research in the field of genetics. Genetic engineering at this time has been widely practiced and the results given are quite destructive.
3. Application of Biochemistry in Food Nutrition Status
Biochemistry has a role in solving nutritional problems in a food that we will manganese. If the food we eat is not enough to have enough nutrition for our daily nutritional needs then the diseases of malnutrition will strike especially susceptible to this disease are children. One of the causes of malnutrition is Food Intake and Infectious Diseases, as has been described above by knowing the reactions that occur in our bodies, we can overcome malnutrition and we will be able to regulate the pattern of food that we will Eating so we can benefit from food optimally. As well as in the application of biochemistry in eating, we are also able to avoid the effects of an environment contaminated by waste that endanger health
hi Aulia, please give me example about vocabulary Organic chemistry?
BalasHapusOrganic chemistry is a branch of scientific studies of the chemistry of the structure, nature, composition, reaction, and synthesis of organic compounds. Organic compounds are built primarily by carbon and hydrogen, and can contain other elements such as nitrogen, oxygen, phosphorus, halogens and sulfur.
HapusThere are many applications of organic chemistry in everyday life, such as in the fields of food, medicine, fuel, coloring, textile, perfume, and so forth.
How is the history of Table Periodic discovery?
BalasHapusThe History of the Periodic Elements System
Hapus1. Grouping Elements by Lavoisier
In 1789, Antoine Lavoiser classified 33 chemical elements. Chemical elements are divided into four groups. Namely gas, soil, metal and non-metals. The gas elements that are grouped by Lavoisier are light, heat, oxygen, azote (nitrogen), and hydrogen.
-The weakness of Lavoisior's theory: Grouping is still too general
2. Grouping of elements according to J.W. Dobereiner
In 1829, J.W. Dobereiner a professor of chemistry from Germany classifies elements based on their similarities.
-The weakness of this theory is the grouping of these elements is less efficient with the presence of several other elements and not included in the triad group when in fact the same with elements in the group of triefd.
3. Grouping of Elements by Chancourtois
In 1862, the French geologist, Alexander Beguyer de Chancourtois, grouped the chemical elements based on atomic weight increases.
4. Newlands Law of Octave
J. Newlands was a British scientist he was the first to classify elements based on relative atomic mass increases. Newlands announced its discovery which is called octave law. He states that the properties of the elements change regularly.
5. Mendeleev periodic system
In 1869 a Russian scholar named Dmitri Ivanovich mendeleev, in the observation of 63 familiar elements, concluded that the properties of the element is a periodic function of the relative atomic mass. That is, if the elements are arranged according to their relative atomic mass increase, certain properties will be repeated periodically.
-The weakness of this theory is that there are still elements whose mass is larger in the presence of a smaller mass element.
6. Modern Periodic System of Henry G. Moseley
In 1913, an English chemist named Henry Moseley conducted an experimental measurement of elemental wavelengths using X-rays. He concludes that the fundamental nature of the atom is not based on relative atomic masses, but based on an increase in the number of protons.
7. Grouping of elements according to Seaborg
In 1940, Glenn Seaborg succeeded in discovering a transuranium element that is an element with an atomic number of 94-102. He broke the placement of these elements by creating a new line so that the modern periodic table changed.