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CHEMISTRY
(CHAPTER 2):
ATOMS, ELEMENTS AND COMPOUNDS - Coggle Diagram
CHEMISTRY
(CHAPTER 2):
ATOMS, ELEMENTS AND COMPOUNDS
ELEMENTS
a substance that cannot be further broken down into simple substances well they are made up of an atom consisting others about atomic particles and a only one type of atom.
EG: SILVER (Ag)
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ATOMS
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ENERGY LEVEL- CONFIGURATION SHELLS, and the energy levels decrease as the shells are drawn farther away from the nucleon
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VALENCY: AMOUNT OF ELECTRONS DONATED OR GAINED TO ATTAIN STABILITY OR STABLE ELECTRONIC CONFIGURATION
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COMPOUNDS
every molecule can't be a compound but every compound is a molecule. compounds and molecules always combined in an equal ratio.
(E.G: H2O)
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MIXTURES
combination of two or more substances that are not chemically joined together and can hence be separated by physical methods of separation. Eg: Salt water, air, sand, blood, sweat and etc.
ISOTOPES
those which are atoms of the same elements which have the same proton number but differ in neutron number which consequently affects the atomic mass
isotopes of the same elements react similarly due to their exact number of protons in the outermost shell.
ISOTOPES:
DEUTRIUM, TRITIUM
ELEMENT:
HYDROGEN
IONIC BOND
IONIC STRUCTURE
the eye answer back together in a regular arrangement of alternating positive and negative ions called a lattice. a regular pattern of lattice of alternating positive and negative ions.
EG: EACH SODIUM IS SURROUNDED BY 6 CHLORIDE IONS AND VICE VERSA, THE SIZE DIFFERS THE structure.
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COVALENT BOND
COVALENT STRUCTURE
compounds containing covalent bonds have molecules to structures can be classified as either simple molecular or giant covalent simple molecular structures are simple formed from only a few items they have strong covalent bonds between the atoms with in a molecule known as intermolecular bonds but have weak bonds between the molecules known as intermolecular forces
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GIANT COVALENT STRUCTURE
graphite is an excellent example of giant covalence structures this is a layer of structure within each layer each carbon atom is bonded to the three other by strong covalent bonds each layer is there for like a giant molecule between is layers there are we causes of attraction and so the layers will pass over each other easily only three covalent bonds formed between carbon atoms within the layers and undered electron is present on each carbon atom the spear or delocalised electrons form electron clouds between the layers and it is because of these pair electrons that graphite conduct electricity peculiarly unlike other covalent bond molecules
diamond structures are also carbon atoms in the giant structure which are covalently bond to four other carbon atoms the former tetrahedral arrangement similar to that a found in silicon oxide this bonding scheme gives rise to very registry dimensional structure and accounts for the extreme hardness of the substances all the outer shell electrons of the carbon atoms are used to form covalent bonds so there are no electrons available to enable diamond to conduct electricity unlike graphite does it is possible to manufacture the different electrodes of carbon diamond is made artificially from graphite at about 300 Celsius at a very high pressure.
atoms can forms table compounds by sharing the electrons in their outermost shells this occurs between non metal atoms, and the bond formed is called a covalent bond
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METALLIC BONDING
PROPERTIES OF METALS
they mostly conduct electricity due to the mobile electrons within the metal structure when a metal is connected in a circuit the electrons move towards the positive terminal while at the same time electrons of fed into the other end of the metal from the negative.
they are malleable and ductile unlike the fixed bonds in diamond metallic bonds are not rigid but they are still strong if a force is applied to a metal rows of ions can slide over one another reposition themselves and the strong bonds reform. malleable primarily means that the metals can be bent or hamered into different shapes. ductile means that the metals can be pulled out into thin wires.
the usually have high melting point and boiling points due to the strong attraction between the positive metal ions and the mobile sea of electrons
in which atoms obtained a more stable electronic configuration that are mostly found in metals. electrons in the outermost shell of the atom of a metal move freely throughout the structure the localised forming a mobile c of electrons when the metal atoms lose these electrons the former giant lattice of positive ions the four metals consists of positive ions embedded in a c of moving electrons the negatively charged electrons attract all the positive metal ions and bond them together with strong electrostatic forces of attraction as a single unit this is a metallic bond.
ATOMIC MASS: the mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number
ATOMIC RELATIVE MASS: the weight in grams of the number of atoms of the element compared to that of carbon-12.
RELATIVE FORMULA MASS: the sum of the relative atomic masses of the atoms in the numbers shown in the formula
STOICHIOMETRY:involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data. In Greek, stoikhein means element and metron means measure, so stoichiometry literally translated means the measure of elements.
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BALANCING EQUATIONS:A balanced equation is an equation for a chemical reaction in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products. In other words, the mass and the charge are balanced on both sides of the reaction.
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