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WorksheetsSK015 Pre-UPS II #2
Total questions: 20
Worksheet time: 5hrs 0mins
The succesive ionisation energies of an element are given as: 760 (first), 1540, 3300, 4399, 8950, and 11900 kJ/mol. From these data alone, it can be inferred that the element...
...is a p-block element
...is a d-block element
...is an s-block element
...has half-filled p orbitals
The number of electrons in the 3d orbitals of the element with a proton number of 26 is...
6
5
4
3
Which of the following pairs of ions have the same electronic configuration? (Proton numbers: Mn=25; Fe=26; Co=27)
Fe3+ and Mn2+
Fe2+ and Mn2+
Fe2+ and Co2+
Mn2+ and Co2+
The boiling point of butanone (CH3CH2COCH3) is higher than that of pentane (CH3CH2CH2CH2CH3) because...
...butanone is polar but pentane is non-polar.
...butanone forms intermolecular hydrogen bonds but pentane does not.
...the covalent bonds in butanone are stronger than the covalent bonds in pentane.
...the dipole-dipole attractions in butanone are stronger than in pentane.
Which of the following contains a set of substances with different chemical bonds?
Aluminium chloride, sodium chloride, mercury
Magnesium, lead, brass
Ethanol, water, ammonia
Nickel (II) chloride, barium nitrate, sodium hydroxide
The electronegativities of some atoms are given: H=2.1; C=2.5; Cl=3.0; O=3.5; F=4.0. Which of the following bonds are the most polar?
C-F
O-F
Cl-H
F-F
The boiling points of water and ammonia are 373 K and 240 K respectively. The boiling point of water is higher than that of ammonia because...
...the hydrogen bonds between water molecules are stronger than the hydrogen bonds between ammonia molecules.
...oxygen is more electronegative than nitrogen.
...the O-H bond in H2O is stronger than the N-H bond in NH3.
...a water molecule has a larger size than an ammonia molecule.
Hydrogen bonds exist in...
liquid ammonia
liquid methane
liquid hydrogen fluoride
Which of the following statements is/are correct?
The boiling point of PH3 is lower than the boiling point of ammonia because there is no hydrogen bonding in PH3.
Pure hydrogen fluoride is a liquid at 273 K because hydrogen-fluorine bond in HF molecule is very strong.
Simple covalent compounds melt at low temperatures because the covalent bonds in them are weak.
Aluminium chloride exists as Al2Cl6 molecules in the gaseous state. From the formula of Al2Cl6, it can be inferred that each aluminium atom...
...forms dative covalent bonds.
...is surrounded by four chlorine atoms arranged tetrahedrally.
...contributes electrons to form four covalent bonds.
The London dispersion forces play an important role in influencing the physical properties of...
CO2 (s)
Mg (s)
NH3 (l)
SiO2 (s)
Which of the following pairs contains molecules that both have a linear geometry?
CS2 and XeF2
SCl2 and SO2
CS2 and SCl2
XeF2 and SO2
Compounds X and Y are simple covalent molecules. They have the following properties:
Compound X has a lower boiling point than Compound Y.
The same type of intermolecular attraction exists in compounds X and Y.
Compound X and Y could be...
X=NH3 and Y=HF
X=HCl and Y=HF
X=HI and Y=HCl
X=H2O and Y=CH4
The figure shows the succesive ionisation energies of an element. The sixth ionisation energy is very much higher than the fifth ionisation energy. This is because...
...the sixth electron is in the inner shell that is filled.
...the sixth electron is nearer to the nucleus.
...the sixth electron is in the outermost shell.
...of the screening effect of the inner electrons.
Which one of these metals has the highest boiling point?
Al
Na
Mg
Li
Which one of these metals has the strongest metallic bond?
Al
Mg
Li
Na
The electronic configuration of Element ZZ is shown as:
1s22s22p63s23p63d104s24p2
What is the position of the element in the periodic table?
Period=4 & Group=14
Period=4 & Group=4
Period=3 & Group=14
Period=4 & Group=12
Why does going down Group 2 the atomic radii increase?
This is due to the increasing in shielding effect when the effective nuclear charges stay constant.
This is due to the increasing in shielding effect when the effective nuclear charges decrease.
This is due to the increasing in effect nuclear charge when the shielding effect is increasing.
This is due to the increasing in effect nuclear charge when the shielding effect is constant.
Going down a group in the periodic table...
...electronegativity decreases.
...the metallic properties increase.
...ease of cation formation increases.
Identify the element with the highest melting point.
Al
Mg
Na
Si
