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WORKSHEET OF CHEMISTRY
CHEMICAL BONDING
By: Dasianto, S.Pd
SMA BRAWIJAYA SMART SCHOOL MALANGJl. CIPAYUNG 10 MALANG
1
CHEMICAL BONDING
A. Differentiating Kinds of Chemical BondingTo understanding differenciation kinds of chemical bonding, do the experiment:
1. Tittle: Differentiating kinds of chemical bonding2. Purpose: Differentiating kinds of chemical bonding using boling point and electrical conductivity3. Tools and equipment
Tools Equipment Termometer Sugar crystalBeaker glass Salt crystalElectrolyte tools kit Water Bunsen burnerGraduated cylinderDigital scale
4. Procedurea. Boiling point
- weigh 5 grams of sugar and 5 grams of salt - dissolve into 50 ml of water in different beaker glass- take 10 mL of solution and bring to the boil- measuring the temperature required until boiling solution
b. Electrical conductivity- Take 10 ml of solution- measure the electrical conductivity of the electrolyte tools kit
5. Experiment dataBoiling point of Conduction of electricity
Sugar solution: Sugar solution: able/notSalt solution: Salt solution: able/not
6. Data AnalysisNo. Questions Answer 1 Which solution which has a higher boiling point?2 Which solution that can conduct electric current?
(Electric current is marked with flashing lights or bubbles formed around the carbon rod)
3 Sugar is one example of covalent compounds. While salt is one example of ionic compounds. In general how the tendency of the boiling point of ionic compounds and covalent compounds? Why its happen?
4 Sugar is one example of covalent compounds. While salt is one example of ionic compounds. In general how the tendency of electrical conductivity of ionic compounds and covalent compounds? Why its happen?
7. ConclussionBased on the experimental results, the tendency of ionic compounds can/cannot conduct the electrical current and the boiling point is higher/lower than covalent compounds.
Additional information: The following data are presented on the differences properties of ionic and covalent compounds:
No Properties Ionic Compounds Covalent CompoundsNon polar Polar
1 Melting/boiling point High Low High 2 Electrical conductivity Solid phase: not conducted
Liquid and solution phase: conducted
Solid phase, liquid phase, solution phase: not conducted
Solid phase, liquid phase,: not conductedsolution phase: conducted
3 Solubility in water Soluble Insoluble soluble
Based on the explanation above, issues that arise are: why the properties of ionic compounds and covalent compounds are different? Why it is happen? The following will be explained about ionic and covalent compounds in detail.
B. Ionic CompoundsIonic compounds are compounds formed by the ionic bonding. Interaction or ionic bonding are attractive forces between positive ions (cations) and negative ions (anions). Cation is an atom or group of atoms positively charged, while the anion is an atom or group of atoms that are negatively charged.There are two types of cations, namely simple cations (formed by removing an electron atoms) and complex cation (group of atoms with a positive charge). As well as anions, simple anion formed by electron accept by atoms, while anion complex is a group of atoms with negative charge. The following examples of cations and anions is accompanied by its name:
Simple cationsGroups
IAName of cations Groups
IIAName of cations Groups
IIIAName of cations
Li+ Litium ion Mg2+ Magnesium ion Al3+ Aluminum ionNa+ Sodium ion Ca2+ Calcium ion Ga3+ Galium ionK+ Potassium ion Sr2+ Stronsium ion
Rb+ Rubidium ion Ba2+ Barium ionCs+ Ceasium ion
Another simple anion with severals chaerges:Cation Name of cations Cation Name of cations
Cu+ Copper(I) ion Sn2+ Tin(II) ionCu2+ Copper(II) ion Sn4+ Tin(IV) ionFe2+ Iron(II) ion Co2+ Cobalt(II) ionFe3+ Iron(III) ion Co3+ Cobalt(III) ion
Complex Cation: NH4+ (ammonium ion)
Simple anionsGroups
VAName of anions Groups
VIAName of anions Groups
VIIAName of anions
N3- Nitride ion O2- Oxide ion F- Fluoride ionS2- Sulfide ion Cl- Chloride ion
Se2- Selenide ion Br- Bromide ionI- Iodide ion
Complex anions(-1) Name of anions (-2) Name of anions (-3) Name of anionsNO2
- Nitrous ion SO32- Sulphite ion PO3
3- Phosphite ionNO3
- Nitrate ion SO42- Sulphate ion PO4
3- Phosphate ionOH- Hydroxide ion CO3
2- Carbonate ionC2O4
2- Oxalate ion CrO4
2- Chromate ionCr2O7
2- Dichromate ion
Based on data above, there are four types of ionic compound:1. Combination between simple cation and simple anion. Example: Na+ + Cl- NaCl (sodium chloride)2. Combination between simple cation and complex anion. Example: Na+ + NO3
- NaNO3 (sodium nitrate)3. Combination between complex cation and simple anion. Example: NH4
+ + Cl- NH4Cl (ammonium chloride)
4. Combination between complex cation and complex anion. Example: NH4+ + NO3
- NH4NO3 (ammonium nitrate)
Exercise: fullfill the folowing table:Cation/anion Cl-
Chloride ionS2-
Sulfide ionNO3
-
Nitrate ionSO4
2-
Sulphate ionPO3
3-
Phosphate ion
Na+
Sodium ionMg2+
Magnesium ionNH4
+
Ammonium ion(NH4)2SO4
Ammonium sulphate
Fe2+
Iron(II) ionFeS
Iron(II) sulfideFe3+
Iron(III) ion The type of ionic compounds to be studied further is the first type. The main material is the process of formation, and writing the symbols Lewis.
Formation of Ionic Compounds.The first type of ionic compounds formed from simple cations and simple anions. Simple cation occurs if a metal atom loses or releases a or amount of electrons, and simple anion formed when nonmetal atom accept a or amounts of electrons. Release or accept electrons aims to achieve stability (reach the noble gas configuration). Thus, the ionic compound can be formed by transfer of electrons between metal and non metal atom. Interaction between cation and anion in ionic compound call as ionic bonding. Example: Write formation of NaCl (sodium chloride) process.11Na: [Ne] 3s1 (have a valence electron, to achieve stability by release an electron)17Cl: [Ne] 3s23p5 (have 5 valence electrons, to achieve stability by accept an electron)
Lewis Symbol of: Na Cl NaCl
Exercise: write the formation process and Lewis Symbol of these ionic compounds:No Ionic Compound No Ionic Compound1 19K + 9F to form KF (potassium fluoride) 5 20Ca + 35Br to form CaBr2 (calcium bromide)
2 12Mg + 8O to form MgO (magnesium oxide) 6 13Al + 17Cl to form AlCl3 (aluminum chloride)
3 13Al + 7N to form AlN (aluminum nitride) 7 19K + 7N to form K3N (potassium nitride)
4 37Rb + 16S to form Rb2S (rubidium sulfide) 8 12Mg + 7N to form Mg3N2 (magnesium nitride)
Properties of ionc compounds:1. Melting and boiling point
Alkaly Halide Melting Point (0C)NaF 993NaCl 801NaBr 747NaI 651
From the table above, melting point of ionic compounds tend to have high, because the ionic bonding in this compound is quite strong. In a group from top to bottom, melting point tend to decrease because increasing bonding radii reduce bonding forces.
2. Physical state of ionic compoundIonic compound commonly in solid phase, hard but brittle if struck by hammer. The slight movement of a layer of ion within crystal suddenly places ions of the same charge next to each other, and for that instant there are large repulsive forces that split the solid and crystal of ionic compound shatters.
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A blowis struck
(a) (b) (c)
3. SolubilityIonic compound able to soluble in polar solvent.
4. Electrical conductivityIn the solid state, ionic compounds do not conduct electricity because the attractive force between cations and anions revent the movement of ions through the crystal. When the solid melted, however, the ions become free to move about and the liquid conducts electricity quite well. In solution, all of the ions are become free and electrical conductivity more stronger. NaCl(l) Na+(l) + Cl-(l)NaCl(s) Na+(aq) + Cl-(aq)
C. Covalent CompoundsCovalent compounds are compounds formed by the covalent bonds. Covalent bonding occurs when two or more atoms share electrons (use electrons together). Generally covalent bonds occur between nonmetal atoms. There are four types of covalent bonding:1. Single covalent bond
Example: formation H2 (hydrogen molecule)
2. Doble covalent bondExample: formation O2 (oxigen molecule)
3. Triple covalent bondExample:
4. Coordinate covalent bond
Exercise: draw the formation of covalent compound below!
Chemical Formula Lewis Structure Chemical
Formula Lewis Structure
Cl2(17Cl)
CO2
(6C, 8O)
PCl3(15P, 17Cl)
XeF2
(54Xe, 9F)
NH3
(7N, 1H)BrF5
(35Br, 9F)
SF4 (16S, 9F)
HCN(1H, 6C, 7N)
H2O(1H, 8O)
PCl3(15P, 17Cl)
The above exercises are for simple molecules. To drawing structure of complex molecules such as H2SO4, HNO3, H3PO3, H3PO4 required systematic ways. Step to drawing complex molecules are:1. Determine the central atom2. Determine the skeletal structure3. Count the Total Valence Electron (TVE)4. Place the sigma (single) covalent bond and making the substitute atom to obey octet rule5. Calculate Total sigma electron (TSE) and Total Lone Pair Electron (TLPE)6. Calculate the rest electron (RE). RE = TVE-TSE-TLPE7. Place the rest electron on the central atom8. Making the lowest formal charge for central atom by making phi (double) bonding
Formula to calculate formal charge is: Qf = NA – NLP – ½ NBP
NA = number of valence electron an atom
NLP = number of lone pair electron NBP = number of bonding pair electronExample: determine formal charge of each atom in NH3 moleculeThe molecule structure of NH3 molecule is
Example: Draw the Lewis structure of NH3 molecule1. The central atom is N2. The skeletal structure
H N H
H3. Count the Total Valence Electron (TVE)
TVE = 5 + 3.1 = 84. Place the sigma (single) covalent bond and making the substitute atom to obey octet rule
5. Calculate Total sigma electron (TSE) and Total Lone Pair Electron (TLPE)TSE = 6TLPE = 0
6. Calculate the rest electron (RE). RE = TVE-TSE-TLPERE = 8-6-0 = 2
7. Place the rest electron on the central atom
8. Calculate the formal charge of each atomQf N = NA – NLP – ½ NBP
= 5 – 2 – ½ 6 = 0
Qf H = NA – NLP – ½ NBP
= 1 – 0 – ½ 2 = 0
Exercise: Draw the Lewis symbol of these compound:Chemical Formula Lewis Structure Chemical
Formula Lewis Structure
H2SO4
(1H, 16S, 8O)
HNO3
(1H, 7N, 8O)
Qf N = NA – NLP – ½ NBP
= 5 – 2 – ½ 6 = 0
Qf H = NA – NLP – ½ NBP
= 1 – 0 – ½ 2 = 0
H3PO3
(1H, 15P, 8O)H3PO4
(1H, 15P, 8O)
D. Shape and Polarity of MoleculesBefore discuss about shape and polarity of moleculs, do this experiment:1. Tittle: Identify polarity of molecule2. Purposes: identify polarity of molecule by experiment3. Tools and equipment
Tools and equipments QuantitiesBurette 6Statif 6Ruler/polythene 1Beaker glass 1 (50 ml)Wool 1 sheetAquadest 50 mlKerosene 50 mlPalm oil 50 mlTab water 50 ml
4. ProcedureFigure Activity
Set the burette, statif look like the figure, and then add:1. Aquadest in burette 12. Kerosene in burette 23. Palm oil in burette 34. Tap water
Charge the polythene/ruler by scouring in wool repeatedly
Polythene placed near the drop of liquid, and observes the current of drop of liquid.
5. Experiment data
Liquid The current of drop of liquidBent Not bent
AquadestKerosenePalm oilTap water
6. Data analysisNo Questions Answer1 Which liquid make the current of drop of liquid
bent? And explain why it’s happen!2 Which liquid make the current of drop of liquid
not bent? And explain why it’s happen!3 Explain, how do these molecules have this
properties?7. Conclussion
Based on this experiment, the polar molecules are ....................................... because able to change of current drop liquid. The non polar molecules are ........................................... because not able to change of current drop liquid
Concepts previously learned is to symbolization compounds in two-dimensional media. The fact that there are in nature, each molecule has a different shape, depending on the type of atoms involved. In this section will be learned about the shape and polarity of a molecule. 3D molecular shape describe the shape of a molecule, polarity of molecule can be determine based on the shape of the molecule. Polarity of molecule is a concept to predict the distribution of electrons in a molecule. If the electrons tend to localize, said non-polar molecules. Whereas in case of the spread of the electrons will be polar molecules.
Table below describe shape and polarity of molecules:Coordination number
General formula
Shape of molecule
Geometri Angels Example Polarity
2 AX2 Linear 1800 CO2, BeCl2 Non polar
3 AX3 Trigonal planar 1200 BF3, BCl3 Non polar
3 AX2E “V” shape/ bent
<1200 SO2 Polar
4 AX4 Tetrahedral 109,50 CH4, CCl4 Non polar
4 AX3E Trigonal pyramidal
<109,50 NH3, PCL3 Polar
4 AX2E2 “V” shape/ bent
<109,50 H2O, SCl2 Polar
4 AXE3 Linear 1800 HF, OH- Polar
5 AX5 Trigonal bipyramidal
Axial:900
Equatorial:1200
PF5, PCl5 Non polar
5 AX4E Seesaw Axial:<900
Equatorial:<1200
SF4, SeF4 Polar
5 AX3E2 “T” shapeAxial:<900
ClF3, BrF Polar
5 AX2E3 Linear Axial:1800 XeF2, I3- Non Polar
6 AX6 Octahedral Axial:900
Equatorial:900
SF6, SeF6 Non polar
6 AX5E Square pyramidal
Axial:900
Equatorial:900
BrF5, IF5 Polar
6 AX4E2 Square planar Equatorial:900
BrF4-, XeF4 Non polar
Step to determine shape of molecule and predict polarity of molecule are:1. Draw the Lewis structure of molecule2. Calculate coordination number (CN) and predict shape of molecule
CN = (BEP + LEP)CN = coordination numberBEP = bonding electron pairs around central atomLEP = lone electron pairs around central atom
3. Calculate moment dipole (µ). Moment dipole is vector resultant of bond in molecule.
Example: Predict shape and polarity of ammonia (NH3)1. Lewis structure of ammonia is
2. CN of ammoniaCN = BEP + LEPCN = 3 + 1CN = 4Shape of molecule:
(trigonal pyramide)3. Moment dipole (µ) of molecule
HH
NH
..
this is polar molecule
Exercise: predict shape and polarity oh these molecules:Chemical Formula Shape and polarity Chemical
Formula Shape and polarity
Cl2(17Cl)
CO2
(6C, 8O)
PCl3(15P, 17Cl)
XeF2
(54Xe, 9F)
NH3
(7N, 1H)BrF5
(35Br, 9F)
SF4 (16S, 9F)
HCN(1H, 6C, 7N)
H2O(1H, 8O)
PCl3(15P, 17Cl)
Properties of covalent compoundsNo Properties Covalent Compounds
Non polar Polar 1 Melting/boiling point Low High 2 Electrical conductivity Solid phase, liquid phase,
solution phase: not conducted
Solid phase, liquid phase,: not conductedsolution phase: conducted
3 Solubility in water (polar solvent) Insoluble Soluble
4 Solubility in CCl4 (non polar solvent) Soluble Insoluble
E. Metallic BondingMetalic bonding is a bond that occurs due to the interaction between the metal atoms. In the electron-sea model, crystal of metal is viewed as 3-dimensional array of metal cations immersed in a sea of delocalized electrons that are free to move throughout the crystal as shown below:
Atom in metallic solid pack closely together in regular structure, if the atoms in metal are represented as spheres, they can only touch the others spheres, and leaving gaps or called as interstitial sites. Amounts of atoms that surrounding an atom called coordination number. Give attention to these pictures:
(a) (b) (c)
Packing of atoms in metals, can be describe in three kinds, they are: hexagonal close packed (HCP), cubic close packed (CCP) and body centered cubic (BCC). Filled this table below!
Type packing atom in metals Picture Explanation
Hexagonal close packed (HCP)
The unit cell of HCP
Coordination number:
How to determine coordination number based on this picture?
A, b, c describe the unit cell. What is the unit cell?
Cubic close packed (CCP)
Coordination number
The unit cell of CCP
Body centered cubic (BCC)
Primitive cubic
Coordination number:
Coordination number:
Properties of metallic bondingIn generall, properties of metals are: dense, malleable and ductile, conductor of heat and electricity, have high melting and boiling point, and lustrous. Give attention the this table:
No Metals Melting Point (0C) Boiling Point (0C)
1 Li 180 1330
2 Na 97.8 890
3 K 63.7 774
4 Na 97.81 892
5 Mg 651 1107
6 Al 660 2467
1. Based on the table, melting/boiling point metals in a group (data no. 1-3) tend to ............................... because .........................................................
2. Based on the table, melting/boiling point metals in a period (data no. 4-6) tend to ............................... because .........................................................
F. Intermolecular ForcessIonic bonding, covalent bonding and metallic bonding are types of intermolecular force. Intermolecular force are interaction between atoms in a molecul. If there are two or more molecule interact each others, called as intermolecular force. So, intermolecular force present on covalent bonding. There are four kinds of intermolecular force:1. London Force
London force occurs when two or more non-polar molecules interact with each other. Example: interaction between H2 and H2, CH4 and H2 etc. Explanation about London force are:
+ _
Molecule withinstantaneous
dipole
++
__
Molecule withinstantaneous
dipole in differentlocations
and so on
++ __Molecule withinstantaneous
dipole
Induction
+ _Molecule withinstantaneous
dipole+ _ Molecule with
induceddipole
Nonpolarmolecule
Instantaneous dipole-induced dipole forceor
London dispersion force
2. Dipole-induced dipole forceDipole-induced dipole force occurs when polar molecule and non polar molecules interact with each other. Example: interaction between HCl and H2, HCl and CH4 etc. Explanation about dipole-induced dipole force are:
+
Induction
Polar moleculewith permanentdipole moment
Nonpolarmolecule
Nonpolarmoleculewith induceddipole
Dipole-induced dipole force
+ +Polar molecule
with permanentdipole moment
_
_ _
_+
3. Dipole-dipole forceDipole-dipole force occurs when two or more polar molecules interact with each other. Example: interaction between HCl and HCl, HCl and CH3Cl etc. Explanation about dipole- dipole force are:
+- +- +- +-
+ -+ -+ -+ -
+- +- +- +-4. Hydrogen bonding
Hydrogen bonding occurs when an atom have hydrogen atom and interact with F, O, N atom from another molecule. Example: interaction between H2O and H2O, H2O and HF, H2O and NH3 etc. Explanation about hydrogen bonding are:
O
HH
OH
H
Hydrogen bond
H
H
FF
Hydrogen bond
202 pm
96 pm
187 pm
92 pm
104.5o
120o 115o
Hydrogen bond
H
H
H
H
HH
NN
The following is the strengthes of intermolecular forces: London < dipole-induced dipole < dipole-dipole < hydrogen bonding.
Effect intermolecular force to physical properties of compounds1. Melting or boiling point
a. the stronger the intermolecular forces the higher boiling point
b. the stronger the London force in non-polar molecule, higher boiling pointMolecules
formulaName of
compoudsMelting
point (oC)Mass
molecule reltifBoiling
point (oC)Physical state at
room temperatureCH4 metana -181,9 16 -163,9 GasC2H6 Etana -183,2 30 -88,5 GasC3H8 Propana -189,6 44 -42,0 GasC4H10 Butana -138,3 58 -0,4 GasC5H12 Pentana -129,9 72 36,2 Cair
2. DensityThe stronger the intermolecular forces, the higher the viscosity of the compound
G. Evaluation 1. Berikut ini yang merupakan kumpulan senyawa
ionic adalah…a. HCl, NaCl, HNO3 d. O3, NO2, BeCl2b. KCl, NaCl, NH4NO3 e. KNO3, BeCl2, KFc. NH3, SO2, CH4
2. Diketahui beberapa jenis ion sebagai berikut: NH4+,
SO42-, Ca2+, PO4
3-, NO3- dan Al3+, maka rumus kimia
senyawa berikut yang tidak benar adalah....a. (NH4)2SO4 c. (NH4)3NO e. AlPO4
b. CaSO4 d . Al2(SO4)3
3. Di antara kelompok senyawa di bawah ini yang semuanya mempunyai ikatan kovalen adalah ....a. KCl, NaCl dan HCl d. NH3, CaO dan K2Ob. HCl, SO2 dan NH3 e. KBr, NaCl dan CaBr2 c. H2O, Na2O dan N2O5
4. Jika unsur Q (Ar = 24) dengan jumlah netron 12 berikatan dengan unsur R (Ar = 35) yang mempunyai jumlah netron 18, maka senyawa yang terbentuk adalah….a. QR2, ikatan ionic d. Q2R, ikatan ionikb. QR2, ikatan kovalen e. QR, ikatan kovalenc. Q2R, ikatan kovalen
5. Berikut ini adalah rumus elektron dari ion nitrat
Ikatan kovalen koordinat pada gambar tersebut ditunjukkan oleh anak panah huruf…a. P c. Q e. Rb. S d. T
6. Sebuah atom netral X mempunyai konfigurasi: [Ne] 3s23p5. Jika unsure tersebut membentuk hidrida, maka senyawa yang mungkin adalah…
a. XH2, ionic c. XH, kovalen e. XH2, kovalen
b. XH, ionic d. XH3, kovalen
7. Unsur A mempunyai massa atom 27 dan memiliki 14 neutron. Unsure B mempunyai 16 neutron dan 16 proton. Jika keduanya berikatan, maka senyawa tersebut memiliki massa molekul relative sebesar…
a. 59 c. 76 e. 150b. 74 d. 86
8. Di dalam senyawa NH4Cl terdapat…a. Ikatan ionikb. Ikatan kovalenc. Ikatan kovalen dan ionicd. Ikatan kovalen dan kovalen koordinasie. Ikatan ionic, kovalen dan kovalen koordinasi
9. Tabel berikut menunjukkan sifat senyawa Q dan R
Senyawa Titik leleh (oC)
Daya Hantar ListrikLelehan Larutan
Q -115 Tidak Mampu R 810 mampu Mampu
Dari data tersebut, ikatan yang terdapat dalam senyawa Q dan R berturut-turut adalah…a. Kovalen polar dan ionb. Kovalen non polar dan ionc. Kovalen non polar dan kovalen polard. Kovalen koordinasi dan ion
e. Kovalen non polar dan hydrogen
10.Diberikan beberapa rumus molekul dan nama masing-masing molekul. Pasangan rumus molekul dan nama yang benar adalah….a. PBr3 = fosfor bromidab. NCl3 = nikel trikloridac. Cl2O7 = klorida pentoksidad. P2O5 = difosfor pentoksidae. SF6 = sulfida heksaflurida
11.Pasangan rumus kimia senyawa yang terbentuk dari ion-ion serta namanya yang benar adalah ....a. Cu2(PO4)3: Tembaga(II) pospatb. Cu(SO4)2 : Tembaga(II) sulfat c. Fe3(PO4)2 : Besi(III) pospatd. Fe2(SO4)3 : Besi(III) sulfate. K2SO4 : Kalsium sulfat
12.Bentuk molekul yang mungkin untuk molekul NH3 adalah (7N, 1H)…
13.Senyawa berikut yang dapat membentuk ikatan hydrogen adalah…
1. H2O (nomor atom O = 6, H = 1)2. CH3OH (nomor atom O = 6, H = 1, C = 6)3. HF (nomor atom F = 9, H = 1)4. HBr (nomor atom Br = 35, H = 1)
14.Senyawa berikut yang memiliki gaya dipole-dipole sebagai gaya antar molekul terkuatnya adalah…
1. H2O (nomor atom O = 6, H = 1)2. CH3Cl (nomor atom Cl = 17, H = 1, C = 6)3. HF (nomor atom F = 9, H = 1)4. HBr (nomor atom Br = 35, H = 1)
15.Tabel berikut menunjukkan sifat senyawa Q dan R
Senyawa Titik leleh (oC)
Daya Hantar ListrikLelehan Larutan
Q -115 Tidak Mampu R 810 Mampu Mampu
Dari data tersebut, ikatan yang terdapat dalam senyawa Q dan R berturut-turut adalah…a. Kovalen polar dan ionb. Kovalen non polar dan ionc. Kovalen non polar dan kovalen polard. Kovalen koordinasi dan ione. Kovalen non polar dan hydrogen
16.Perhatikan gambar berikut:
Ikatan/interaksi antar molekul yang ditunjukkan nomor 3 adalah....a. Gaya dipol-dipol induksib. Gaya dipol-dipolc. Ikatan hidrogend. Gaya Londone. Gaya ion-dipol
17.Apabila unsur 16X berikatan dengan unsur 35Y, maka rumus kimia dan jenis ikatan yang terbentuk adalah...
a. XY ionik c. XY2 ionik e. X2Y kovalen
b. X2Y ionik d. XY2 kovalen
18.Rumus kimia dan jenis ikatan yang terjadi jika 20Ca berikatan dengan unsure Z adalah…
a. CaZ2, kovalen d. CaZ2, ionik
b. Ca2Z, kovalen e. Ca2Z, ionik
c. CaZ, ionik
19.Senyawa yang tersusun dari buah unsure 6X dan 17Y, bila berikatan akan memiliki bentuk molekul dan dan kepolaran berturut-turut adalah…
a. Tetrahedral, polar d. bentuk V, non polar
b. Tetrahedral, non polar e. Bentuk V, polarc. Trigonal bipiramida, polar
20.Berikut ini adalah rumus elektron dari ion nitrat
Ikatan kovalen koordinat pada gambar tersebut ditunjukkan oleh anak panah huruf…c. P c. Q e. Rd. S d. T
21.Perhatikan grafik titik didih beberapa senyawa hidrida golongan IV-A, V-A, dan VI-A berikut ini! (UN 2013)
Senyawa yang mempunyai ikatan hidrogen antar molekulnya adalah nomor...a. 1 dan 2 c. 1 dan 3 e. 4 dan 5b. 4 dan 6 d. 5 dan 6
22.Perhatikan data hasil percobaan berikut.
No Sifat fisik Zat A Zat B1 Wujud zat Padat Padat2 Kelarutan dalam air Larut Tidak larut3 Daya hantar listrik
larutanKonduktor Isolator
4 Titik leleh dan titik didih Tinggi RendahBerdasarkan data tersebut, dapat disimpulkan bahwa jenis ikatan yang terdapat pada zat A dan zat B berturut-turut adalah….A. ionik dan kovalen nonpolarB. kovalen polar dan ionikC. kovalen nonpolar dan ionikD. kovalen koordinasi dan logamE. hidrogen dan kovalen
