Question
If 
and 
are 
such that 
where ‘O’ is the origin, then the d.c.’s of the internal bisector of the angle 
are
The correct answer is:
Let OA and OB be two lines with d.c’s 
. Then, the coordinates of A and B are 
respectively. Let OC be the bisector of 
. Then, C is the mid point of AB and so its coordinates are 
.
We have, 
Related Questions to study
The area bounded by the curves is 
and 
(where a 
is
The area bounded by the curves is and (where a is
The electronic configurations of the element A,B, and C are :given below.
The bond between B and C will be:
The electronic configurations of the element A,B, and C are :given below.
The bond between B and C will be:
The electronic configurations of the element A,B, and C are :given below.
The molecular formula of the compound formed from Band C will be:
The electronic configurations of the element A,B, and C are :given below.
The molecular formula of the compound formed from Band C will be:
The electronic configurations of the element A,B, and C are :given below.
Stable form of C may be represented by the formula:
The electronic configurations of the element A,B, and C are :given below.
Stable form of C may be represented by the formula:
The electronic configurations of the element A,B, and C are :given below.
Stable form of A may be represented by the formula:
The electronic configurations of the element A,B, and C are :given below.
Stable form of A may be represented by the formula:
Lewis concept of covalency of an element involvesoctetrule.Lateronitwasfoundthatmanyelementsin their compounds, e.g., 
etc. have incompleteoctetwhereas
et c.haveexpandedoctet. This classical concept also failed inpredictingthegeometryof molecules. Modem concept of covalence was pro posed in terms of valence bond theory. Hybridizationconcept along with valence bond theory successfully explained the geometryofvariousmoleculesbutfailedin many molecules Thebondangle
and
are,respectively:
Lewis concept of covalency of an element involvesoctetrule.Lateronitwasfoundthatmanyelementsin their compounds, e.g., etc. have incompleteoctetwhereas et c.haveexpandedoctet. This classical concept also failed inpredictingthegeometryof molecules. Modem concept of covalence was pro posed in terms of valence bond theory. Hybridizationconcept along with valence bond theory successfully explained the geometryofvariousmoleculesbutfailedin many molecules Thebondangleandare,respectively:
NO is a colorless gasandan important intermediate inthemanufactureof nitricacidby catalytic oxidationofammonia. Whichofthefollowingisaneutraloxide?</span
NO is a colorless gasandan important intermediate inthemanufactureof nitricacidby catalytic oxidationofammonia. Whichofthefollowingisaneutraloxide?</span
NO has11 valence electrons.It is impossible for all10 be paired. and hence this is an odd electron molecule,and the gas is paramagnetic. Which of the following species has the smallest N-O bond length?
NO has11 valence electrons.It is impossible for all10 be paired. and hence this is an odd electron molecule,and the gas is paramagnetic. Which of the following species has the smallest N-O bond length?
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series. Which has the smallest bond angle 
in the given molecules?
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series. Which has the smallest bond angle in the given molecules?
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series.
Consider the following hydrides and arrange them in increasing order of bond ang les:
I) 
II) 
III) 
IV) 
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series.
Consider the following hydrides and arrange them in increasing order of bond ang les:
I)
II)
III)
IV)
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series. Consider the following molecules:
I) 
II) 
III) 
IV) 
Arrange these molecules in increasing order of bond angle:
Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond ang les. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series. Consider the following molecules:
I)
II)
III)
IV)
Arrange these molecules in increasing order of bond angle:
three resonance structures are consistent with the electron -dot method Structure A has only one negative formal charge on the nitrogen atom, the most electro negative atom in the ion. Structure B has a single negative charge on the S, which is less electronegative than N. Structure C has charges of -2 on N and +1 on S, consistent with the relative electronegativities of the atoms but with a larger charge and greater charge separation than the first.
bonds 
bonds in the following structure is:
