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atomic structure (Atomic structure (difference between an atom and an ion…

- - - - monotomic ions vs. poliatomic ions
        
        polyatomic ions:
        
        mono = 1
        
        single atoms that has lost / gained electrons (ionic bonding)
        
        have subscript numbers
        
        examples; Cl- or Cu2+ or Al3+
        
        monatomic ions:
        
        poly = many
        
        group of atoms that has lost / gained electrons
        
        atoms held together by sharing electrons (covalent bonding)
        
        have subscript numbers and superscript numbers
        
        examples; NO3 - or CO3 2-
      - Basic ions, their formula & charges:
        
        ammonium ion = NH4 +
        
        sodium ion = Na +
        
        potassium ion = K +
        
        silver ion = Ag +
        
        hydrogen ion = H +
        
        calcium ion = Ca2 +
        
        zinc ion = Zn 2+
        
        alumium ion = Al 3+
        
        iron (II) / ferous ion = Fe 2+
        
        iron (III) / ferric ion = Fe 3+
        
        magnesium ion = Mg 2+
        
        Copper ion = Cu 2+
        
        lead ion = Pb 2+
        
        barium ion = Ba 2+
        
        oxide ion = O 2-
        
        sulfide ion = S 2-
        
        carbonate ion = CO3 2-
        
        solfate ion = SO4 2-
        
        hydroxide ion = OH -
        
        chloride ion = Cl -
        
        nitrate ion = NO3 -
        
        hydrogen carbonate / bicarbonate ion = HCO3 -
        
        steps by witch the ions are formed, some examples;
        Calcium atom:
        
        symbol = Ca
        
        atomic number = 20
        
        electron arangement = 2,8,8,2
        
        electrons arrangement of ion = 2,8,8, (it has lost 2 elelctrons to ave a full valence shell -2)
        
        ion symbol/charge = Ca2+
        
        Florine atom:
        
        symbol = F
        
        atomic number = 9
        
        elelctron arrangement = 2,7
        
        electron arrangement of ion = 2,8 ( it has gained 1 elelctron, to fill the valence shell +1)
        
        ion syble = F-
        
        how to write; formation of ions in relation to electron arrangement and no. of protons and electrons
        
        example: (Calcium)
        Calcium atom (Ca) has 20 protons and 20 electrons, with an electron arrangement of 2,8,8,2. the atom must loose 2 electrons in order to have a full valence shell. the calcium ion will now have 2 more protons that electrons, and therefor have a positive charge of 2+. the ion has only 18 electrons and an electron arrangement of 2,8,8. it has a positive charge and is therefore a cation. calcium is in group 2, group 2 elements are generaly quite unstable as it has such an empty valce shell, however clacium ion is now stable.
        
        what to include:
        
        group number
        
        protons and electron arrangement of atom
        
        protons and electron arrangement of ion
        
        charge & if its a cation/anion
        
        ( Cl- & Ca2+ bothe now have the same electron configuration of 2,8,8
        
        rules for the names of ions
        
        ides are all monoatomic &ates are all polyatomic +contian oxygen
        
        the name of simple positive ions have the same name as the atoms they are formed forme
        
        the name of simple negative ions change the atom name to the end into -ide
        
        the name of a negative ion with a polyatomic ion changes the nae of the atom to end in -ate (has oxygen in it)
        
        ways ion charges are written:
        
        charge of the ion = superscript (top of the symbol)
        
        number of each kind of atom in an ion (polyatomic ions)
        = subscript (bottom of symbol) - ratio of the different elements in the substance
      - there are two types of ions; cations (+) and anions (-)
        
        anions (-) :
        
        anions have a negative charge (-)
        
        anions have gained electrons , therefor have more electrons than protons.
        
        the difference between cations(+) and anions(-), is their net electrical charge (they are both ions)
        
        metals vs. non metals
        
        non-metals = generally have a large number of valence electrons ( 5,6,7,8). so atoms require gaining electerons to create ions, this gives them a negative charge (anions -)
        
        metals = generally have small no. of valence electrons (1,2,3). so atoms require losing electrons to create their ions, this gives them a positive charge (cations +)
        
        cations (+):
        
        cations have a positive charge (+)
        
        cations have lost electrons, this means there are more protons than electrons
    - - E = Electrons
        B = Bend
        C = Charge
        R = Ratio
        E:
        
        Atoms that form compound
        
        electrons lost/gained from those atoms to form the ion
        
        gains/ looses certain amount of electrons to fill the valence shell - witch is a cation/anion
        
        no. of protons & electrons in each ion
        
        every ... reacts with .... of ... to make the compound
        
        B:
        
        bond forming ... compound is an ionic bond
        
        ionic bond, loose, gain, exchange electrons
        
        ... number of electrons gained/lost and given/taken from ... to fill outer shell
        
        attraction between cation & anion, oppositely charged ions
        
        C:
        
        is an ionic substance
        
        (for each) (name) ion is (formula), has charge of ... (... more/less electrons than protons)
        
        ionic substance/compound can't have overall charge (charge of zero)
        
        individual ion charges, that make up compound must cancel each other out
        
        R:
        
        for the compoun (name and formula) there is ... number of this ion & ... number of that
        
        Al3+, Cl,Cl ( example)
        
        tranfers ... electrpns from... ions to ... number of this many ions
        
        to make overall charge of zero ( no charge)
        
        ration written as (example) Al3+ : Cl- is 1:3, for each compound
        
        ration for compound written as subscript, making .... formula
  - - - changing the number of neutrons in an atom doesn't change the element, they are just an isotope of that element, (a type of variation of that element)
  - - - elements = 1 type of atom, all have different structure and properties. an element can't be divided into any smaller/multiple elements
        
        non metals = all elements that aren't metals
        
        typically gas @ room temp. - brittle
        
        low conductivity
        
        right hand side of the periodic table
        
        metals = majority of elements
        
        typically have a solid state @ room temp.
        
        shiny
        
        conduct heat and electricity well
        
        hard density - malleable
        
        left hand side of the periodic table
      - compounds = two or more elements chemically combined
  - - - changes in state are physical changes