A. KATION (ION POSITIF)

Kation adalah muatan positif, yang terbentuk saat atom/molekul kekurangan elektron. Jika atom X melepaskan 1 elektron, akan membentuk ion positif \(\ce{X+}\). Jika atom X melepaskan 2 elektron, akan membentuk ion positif  \(\ce{X^{2+}}\). Dan seterusnya.

Berikut adalah beberapa contoh kation:

	Unsur	Kation	Nama
Golongan IA	\(\ce{Li}\)	\(\ce{Li+}\)	Litium
	\(\ce{Na}\)	\(\ce{Na+}\)	Natrium
	\(\ce{K}\)	\(\ce{K+}\)	Kalium (potasium)
	\(\ce{Rb}\)	\(\ce{Rb+}\)	Rubium
	\(\ce{Cs}\)	\(\ce{Cs+}\)	Cesium
Golongan IIA	\(\ce{Mg}\)	\(\ce{Mg^{2+}}\)	Magnesium
	\(\ce{Ca}\)	\(\ce{Ca^{2+}}\)	Kalsium
	\(\ce{Sr}\)	\(\ce{Sr^{2+}}\)	Stronsium
	\(\ce{Ba}\)	\(\ce{Ba^{2+}}\)	Barium
Golongan IIIA	\(\ce{Al}\)	\(\ce{Al^{3+}}\)	Alumunium
	\(\ce{Ga}\)	\(\ce{Ga^{3+}}\)	Galium
	\(\ce{In}\)	\(\ce{In^{3+}}\)	Indium
	\(\ce{Tl}\)	\(\ce{Tl^{3+}}\)	Talium
Golongan IVA	\(\ce{Sn}\)	\(\ce{Sn^{2+}}\)	Timah (II)
	\(\ce{Sn}\)	\(\ce{Sn^{4+}}\)	Timah (IV)
	\(\ce{Pb}\)	\(\ce{Pb^{2+}}\)	Timbal (II)
	\(\ce{Pb}\)	\(\ce{Pb^{4+}}\)	Timbal (IV)
Golongan B	\(\ce{Ag}\)	\(\ce{Ag+}\)	Perak
	\(\ce{Ni}\)	\(\ce{Ni^{2+}}\)	Nikel
	\(\ce{Cd}\)	\(\ce{Cd^{2+}}\)	Cadmium
	\(\ce{Zn}\)	\(\ce{Zn^{2+}}\)	Seng
	\(\ce{Cr}\)	\(\ce{Cr^{3+}}\)	Kromium
	\(\ce{Pt}\)	\(\ce{Pt^{4+}}\)	Platina
	\(\ce{Cu}\)	\(\ce{Cu^{+}}\)	Tembaga (I)
		\(\ce{Cu^{2+}}\)	Tembaga (II)
	\(\ce{Hg}\)	\(\ce{Hg^{+}}\)	Raksa (I)
		\(\ce{Hg^{2+}}\)	Raksa (II)
	\(\ce{Au}\)	\(\ce{Au^{+}}\)	Emas (I)
		\(\ce{Au^{3+}}\)	Emas (III)
	\(\ce{Fe}\)	\(\ce{Fe^{2+}}\)	Besi (II)
		\(\ce{Fe^{3+}}\)	Besi (III)
	\(\ce{Co}\)	\(\ce{Co^{2+}}\)	Kobalt (II)
		\(\ce{Co^{3+}}\)	Kobalt (III)
Kation lainnya		\(\ce{NH4+}\)	Amonium

B. ANION (ION NEGATIF)

Anion adalah muatan negatif, yang dihasilkan saat atom/molekul kelebihan elektron. Jika atom X menerima 1 elektron, akan membentuk ion negatif \(\ce{X-}\). Jika atom X menerima 2 elektron, akan membentuk ion negatif \(\ce{X^{2-}}\). Dan seterusnya.

Berikut adalah beberapa contoh anion:

	Anion	Nama
Golongan IVA	\(\ce{CO3^{2-}}\)	Karbonat
	\(\ce{SiO3^{2-}}\)	Silikat
Golongan VA	\(\ce{NO2^{-}}\)	Nitrit
	\(\ce{NO3^{-}}\)	Nitrat
	\(\ce{PO3^{2-}}\)	Fosfit
	\(\ce{PO4^{2-}}\)	Fosfat
	\(\ce{AsO3^{2-}}\)	Arsenit
	\(\ce{AsO4^{2-}}\)	Arsenat
	\(\ce{SbO3^{2-}}\)	Antimonit
	\(\ce{SbO4^{2-}}\)	Antimonat
Golongan VIA	\(\ce{O^{2-}}\)	Oksida
	\(\ce{S^{2-}}\)	Sulfida
	\(\ce{SO3^{2-}}\)	Sulfit
	\(\ce{SO4^{2-}}\)	Sulfat
Golongan VIIA	\(\ce{F-}\)	Fluorida
	\(\ce{Cl-}\)	Klorida
	\(\ce{ClO-}\)	Hipoklorit
	\(\ce{ClO2-}\)	Klorit
	\(\ce{ClO3-}\)	Klorat
	\(\ce{ClO4-}\)	Perklorat
	\(\ce{Br-}\)	Bromida
	\(\ce{BrO4-}\)	Bromat
	\(\ce{I-}\)	Iodida
	\(\ce{IO4-}\)	Iodat
Anion lainnya	\(\ce{OH-}\)	Hidroksida
	\(\ce{CN-}\)	Sianida
	\(\ce{CHOO-}\)	Formiat
	\(\ce{CH3COO-}\)	Asetat
	\(\ce{HCO3-}\)	Bikarbonat
	\(\ce{MnO4-}\)	Permanganat
	\(\ce{MnO4^{2-}}\)	Manganat
	\(\ce{CrO4^{2-}}\)	Kromat
	\(\ce{Cr2O7^{2-}}\)	Dikromat

C. SENYAWA IONIK

Senyawa ionik terdiri atas ion positif (kation) dan ion negatif (anion). Penamaan senyawa ionik dimulai dari kation dan diikuti oleh anionnya.

Senyawa	\(\ce{->}\)	Kation	+	Anion	Nama
\(\ce{NaCl}\)	+	\(\ce{Na+}\)	\(\ce{->}\)	\(\ce{Cl-}\)	Natrium klorida
\(\ce{Mg(NO3)2}\)	+	\(\ce{Mg^{2+}}\)	\(\ce{->}\)	\(\ce{2 NO3-}\)	Magnesium nitrat
\(\ce{K2CO3}\)	+	\(\ce{2 K+}\)	\(\ce{->}\)	\(\ce{CO3^{2-}}\)	Kalium karbonat
\(\ce{BaSiO3}\)	+	\(\ce{Ba^{2+}}\)	\(\ce{->}\)	\(\ce{SiO3^{2-}}\)	Barium silikat
\(\ce{Al2(AsO4)3}\)	+	\(\ce{2 Al^{3+}}\)	\(\ce{->}\)	\(\ce{3 AsO4^{3-}}\)	Alumunium arsenat
\(\ce{Ca3(PO4)2}\)	+	\(\ce{3 Ca^{2+}}\)	\(\ce{->}\)	\(\ce{2 PO4^{3-}}\)	Kalsium fosfat
\(\ce{NH4CN}\)	+	\(\ce{NH4^{+}}\)	\(\ce{->}\)	\(\ce{CN-}\)	Amonium sianida
\(\ce{(NH4)2SO4}\)	+	\(\ce{2 NH4^{+}}\)	\(\ce{->}\)	\(\ce{SO4^{2-}}\)	Amonium sulfat
\(\ce{CH3COONa}\)	+	\(\ce{Na+}\)	\(\ce{->}\)	\(\ce{CHOO-}\)	Natrium formiat
\(\ce{Zn(CH3COO)2}\)	+	\(\ce{Zn^{2+}}\)	\(\ce{->}\)	\(\ce{2 CH3COO-}\)	Seng asetat

 

JIKA KATION MEMILIKI LEBIH DARI 1 JENIS MUATAN

Senyawa	+	Kation	+	Anion	Nama
\(\ce{Cu2S}\)	+	\(\ce{2 Cu^{+}}\)	\(\ce{->}\)	\(\ce{S^{2-}}\)	Tembaga (I) sulfida
\(\ce{CuS}\)	+	\(\ce{Cu^{2+}}\)	\(\ce{->}\)	\(\ce{S^{2-}}\)	Tembaga (II) sulfida
\(\ce{Fe(IO4)2}\)	+	\(\ce{Fe^{2+}}\)	\(\ce{->}\)	\(\ce{2 IO4-}\)	Besi (II) iodat
\(\ce{Fe(IO4)3}\)	+	\(\ce{Fe^{3+}}\)	\(\ce{->}\)	\(\ce{3 IO4-}\)	Besi (III) iodat

D. Oksida Logam (Oksida Basa)

Oksida logam atau oksida basa adalah senyawa yang berasal dari unsur logam dan oksigen.

 

\(\ce{UNSUR LOGAM + O2 -> OKSIDA LOGAM (OKSIDA BASA)}\)

Oksida Logam	Nama
\(\ce{Li2O}\)	Lithium oksida
\(\ce{MgO}\)	Magnesium oksida
\(\ce{Al2O3}\)	Alumunium oksida

 

JIKA LOGAM MEMILIKI LEBIH DARI 1 JENIS MUATAN

Oksida Logam	Nama
\(\ce{Cu2O}\)	Tembaga (I) oksida
\(\ce{CuO}\)	Tembaga (II) oksida
\(\ce{FeO}\)	Besi (II) oksida
\(\ce{Fe2O3}\)	Besi (III) oksida

E. SENYAWA KOVALEN

Senyawa kovalen terdiri atas unsur-unsur nonlogam.

Tatanama senyawa kovalen menggunakan aturan sebagai berikut:

• Unsur kedua ditambahkan akhiran "ida"
• Penamaan senyawa kovalen menggunakan awalan sebagai berikut:

Kecuali jika jumlah atom unsur pertama = 1, tidak ditambahkan mono.

 

Contoh:

\(\ce{NF3}\) = nitrogen trifluorida (bukan mononitrogen trifluorida)

\(\ce{PCl5}\) = fosfor pentaklorida (bukan monofosfor pentaklorida)

\(\ce{CO}\) = karbon monoksida (bukan monokarbon monoksida)

\(\ce{Cl2O7}\) = dikloro heptaoksida

F. ASAM

Asam adalah zat yang dalam bentuk larutan melepaskan ion \(\ce{H+}\).

Cara penamaan zat asam adalah asam diikuti dengan nama ion negatifnya.

Asam	Ionisasi	Nama
\(\ce{H2S}\)	\(\ce{2 H+ + S^{2-}}\)	Asam sulfida
\(\ce{HF}\)	\(\ce{H+ + F^{-}}\)	Asam fluorida
\(\ce{HCl}\)	\(\ce{H+ + Cl^{-}}\)	Asam klorida
\(\ce{HBr}\)	\(\ce{H+ + Br^{-}}\)	Asam bromida
\(\ce{HI}\)	\(\ce{H+ + I^{-}}\)	Asam iodida
\(\ce{CHOOH}\)	\(\ce{CHOO^{-} + H+}\)	Asam formiat
\(\ce{CH3COOH}\)	\(\ce{CH3COO^{-} + H+}\)	Asam asetat
\(\ce{H2CO3}\)	\(\ce{2 H+ + CO3^{2-}}\)	Asam karbonat
\(\ce{H2SO3}\)	\(\ce{2 H+ + SO3^{2-}}\)	Asam sulfit
\(\ce{H2SO4}\)	\(\ce{2 H+ + SO4^{2-}}\)	Asam sulfat
\(\ce{HNO2}\)	\(\ce{H+ + NO2^{-}}\)	Asam nitrit
\(\ce{HNO3}\)	\(\ce{H+ + NO3^{-}}\)	Asam nitrat
\(\ce{H3PO3}\)	\(\ce{3 H+ + PO3^{3-}}\)	Asam fosfit
\(\ce{H3PO4}\)	\(\ce{3 H+ + PO4^{3-}}\)	Asam fosfat
\(\ce{H3AsO3}\)	\(\ce{3 H+ + AsO3^{3-}}\)	Asam arsenit
\(\ce{H3AsO4}\)	\(\ce{3 H+ + AsO4^{3-}}\)	Asam arsenat

G. Basa

Basa adalah zat yang dalam bentuk larutan melepaskan ion \(\ce{OH-}\).

Basa	Nama	Ionisasi
\(\ce{LiOH}\)	Lithium hidroksida	\(\ce{Li+ + OH^{-}}\)
\(\ce{Mg(OH)2}\)	Magnesium hidroksida	\(\ce{Mg^{2+} + 2 OH^{-}}\)
\(\ce{Al(OH)3}\)	Alumunium hidroksida	\(\ce{Al^{3+} + 3 OH^{-}}\)
\(\ce{NH4OH}\)	Amonium Hidroksida	\(\ce{NH4+ + OH^{-}}\)

 

JIKA KATION MEMILIKI LEBIH DARI 1 JENIS MUATAN

Basa	Nama	Ionisasi
\(\ce{CuOH}\)	Tembaga (I) hidroksida	\(\ce{Cu^{+} + OH^{-}}\)
\(\ce{Cu(OH)2}\)	Tembaga (II) hidroksida	\(\ce{Cu^{2+} + 2 OH^{-}}\)
\(\ce{Fe(OH)2}\)	Besi (II) hidroksida	\(\ce{Fe^{2+} + 2 OH^{-}}\)
\(\ce{Fe(OH)3}\)	Besi (III) hidroksida	\(\ce{Fe^{3+} + 3 OH^{-}}\)

H. PEMBENTUKAN ASAM DAN BASA

1. Pembentukan Oksida Asam

Oksida asam adalah senyawa yang berasal dari unsur nonlogam dan oksigen.

 

\(\ce{UNSUR NONLOGAM + O2 -> OKSIDA ASAM}\)

Unsur	+	\(\ce{O2}\)	\(\ce{->}\)	Senyawa
B Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{B2O3}\) Diboron trioksida
C Bilangan oksidasi: +4	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{CO2}\) Karbon dioksida
Si Bilangan oksidasi: +4	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{SiO2}\) Silikon dioksida
S Bilangan oksidasi: +4	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{SO2}\) Belerang dioksida
S Bilangan oksidasi: +6	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{SO3}\) Belerang trioksida
N Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{N2O3}\) Dinitrogen trioksida
N Bilangan oksidasi: +5	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{N2O5}\) Dinitrogen pentaoksida
P Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{P2O3}\) Difosfor trioksida
P Bilangan oksidasi: +5	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{P2O5}\) Difosfor pentaoksida
As Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{As2O3}\) Diarsen trioksida
As Bilangan oksidasi: +5	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{As2O5}\) Diarsen pentaoksida
Sb Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Sb2O3}\) Diantimon trioksida
Sb Bilangan oksidasi: +5	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Sb2O5}\) Diantimon pentaoksida

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2. Pembentukan Asam

Asam adalah zat yang dalam bentuk larutan melepaskan ion \(\ce{H+}\).

 

\(\ce{OKSIDA ASAM + H2O -> ASAM}\)

Oksida Asam	+	\(\ce{H2O}\)	\(\ce{->}\)	Asam
\(\ce{CO2}\) Karbon dioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H2CO3}\) Asam karbonat Asam karbonat (IV)
\(\ce{SO2}\) Belerang dioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H2SO3}\) Asam sulfit Asam sulfat (IV)
\(\ce{SO3}\) Belerang dioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H2SO4}\) Asam sulfat Asam sulfat (VI)
\(\ce{N2O3}\) Dinitrogen trioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{HNO2}\) Asam nitrit Asam nitrat (III)
\(\ce{N2O5}\) Dinitrogen pentaoksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{HNO3}\) Asam nitrat Asam nitrat (V)
\(\ce{P2O3}\) Difosfor trioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H3PO3}\) Asam fosfit Asam fosfat (III)
\(\ce{P2O5}\) Difosfor pentaoksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H3PO4}\) Asam fosfat (V)
\(\ce{As2O3}\) Diarsen trioksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H3AsO3}\) Asam arsenit Asam arsenat (III)
\(\ce{As2O5}\) Diarsen pentaoksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{H3AsO4}\) Asam arsenat Asam arsenat (V)

Catatan:

Khusus oksida boron (B), fosfor (P), arsen (As) dan antimon (Sb), ditambahkan 3 molekul \(\ce{H2O}\)

 

ASAM YANG TIDAK MENGANDUNG OKSIGEN

\(\ce{H2}\)	+	Sulfur dan Halogen	\(\ce{->}\)	Asam	Ionisasi
\(\ce{H2}\)	+	\(\ce{S}\) Sulfur	\(\ce{->}\)	\(\ce{H2S}\) Asam sulfida	\(\ce{2 H+ + S^{2-}}\)
\(\ce{H2}\)	+	\(\ce{F2}\) Fluorin	\(\ce{->}\)	\(\ce{HF}\) Asam fluorida	\(\ce{H+ + F^{-}}\)
\(\ce{H2}\)	+	\(\ce{Cl2}\) Klorin	\(\ce{->}\)	\(\ce{HCl}\) Asam klorida	\(\ce{H+ + Cl^{-}}\)
\(\ce{H2}\)	+	\(\ce{Br2}\) Bromin	\(\ce{->}\)	\(\ce{HBr}\) Asam bromida	\(\ce{H+ + Br^{-}}\)
\(\ce{H2}\)	+	\(\ce{I2}\) Iodin	\(\ce{->}\)	\(\ce{HI}\) Asam iodida	\(\ce{H+ + I^{-}}\)

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3. Pembentukan Oksida Basa

Oksida basa adalah senyawa yang berasal dari unsur logam dan oksigen.

 

\(\ce{UNSUR LOGAM + O2 -> OKSIDA BASA}\)

Unsur	+	\(\ce{O2}\)	\(\ce{->}\)	Oksida Basa
\(\ce{Li}\) Bilangan oksidasi: +1	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Li2O}\) Lithium oksida
\(\ce{Mg}\) Bilangan oksidasi: +2	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{MgO}\) Magnesium oksida
\(\ce{Al}\) Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Al2O3}\) Alumunium oksida
\(\ce{Pt}\) Bilangan oksidasi: +4	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{PtO2}\) Platina oksida
\(\ce{Cu}\) Bilangan oksidasi: +1	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Cu2O}\) Tembaga (I) oksida
\(\ce{Cu}\) Bilangan oksidasi: +2	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{CuO}\) Tembaga (II) oksida
\(\ce{Fe}\) Bilangan oksidasi: +2	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{FeO}\) Besi (II) oksida
\(\ce{Fe}\) Bilangan oksidasi: +3	+	\(\ce{O2}\) Bilangan oksidasi: −2	\(\ce{->}\)	\(\ce{Fe2O3}\) Besi (III) oksida

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4. Pembentukan Basa

Basa adalah zat yang dalam bentuk larutan melepaskan ion \(\ce{OH-}\).

 

\(\ce{OKSIDA BASA + H2O -> BASA}\)

Oksida Basa	+	\(\ce{H2O}\)	\(\ce{->}\)	Basa
\(\ce{Li2O}\) Lithium oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{LiOH}\) Lithium hidroksida
\(\ce{MgO}\) Magnesium oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Mg(OH)2}\) Magnesium hidroksida
\(\ce{Al2O3}\) Alumunium oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Al(OH)3}\) Alumunium hidroksida
\(\ce{PtO2}\) Platina (IV) oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Pt(OH)4}\) Platina hidroksida
\(\ce{Cu2O}\) Tembaga (I) oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{CuOH}\) Tembaga (I) hidroksida
\(\ce{CuO}\) Tembaga (II) oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Cu(OH)2}\) Tembaga (II) hidroksida
\(\ce{FeO}\) Besi (II) oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Fe(OH)2}\) Besi (II) hidroksida
\(\ce{Fe2O3}\) Besi (III) oksida	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{Fe(OH)3}\) Besi (III) hidroksida
\(\ce{NH3 (g)}\) Amonia	+	\(\ce{H2O}\)	\(\ce{->}\)	\(\ce{NH4OH (aq)}\) Amonium Hidroksida