Answer:
1) False
2) False
3) True
4) True
5) False
Explanation:
1. Two sigma bonds comprise a double bond: False
Two sigma bonds are not possible between two atoms . There will always be one pi bond or two bonds with one sigma bond
2. A triple bond consists of one pi bond and two sigma bonds.
Two sigma bonds are not possible between two atoms . There will always be one pi bond or two bonds with one sigma bond
3. Bonds formed from atomic s orbitals are always sigma bonds. True
There is always an head to head overlapping possible with s orbital
4. A pi bond restricts rotation about the sigma-bond axis.
True.
5. A pi bond consists of two pairs of electrons.
False
Each bond can have one pair of electrons
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Reactants are on the left side of the arrow, while products are on the right
Answer:
a. The new pressure is 606,25 Torr.
b. -243,9°C is needed to reach the pressure of 7250 Torr.
Explanation:
Gay Lussac's law for gases says that if the volume in a gas remains constant, the pressure will be directly proportional to the temperature change.
P1 . T1 = P2. T2
(Temperature must be in K)
725 Torr . 291 K = P2 . 348 K
(725 Torr . 291 K) /348 K = P2
606,25 Torr = P2
725 Torr . 291K = 7250 Torr . T2
(725 Torr . 291K) /7250 Torr = T2
29,1 K = T2
T° K - 273 = T°C
29,1 K -273 = -243,9°C
The correct answer is higher melting point, bound by metal metal bonds.
While alkali metals only have one valence electron, alkaline earth metals have two. Metal to metal connections hold the metals together. Alkaline earth metals have a stronger metallic connection and a higher melting point because they have two valence electrons.
the characteristics that Group 2 metals excel in over Group 1 metals.
- Initial Ionization Potential
- Group 2 items are more difficult than group 1 elements.
- Strong propensity to produce bivalent compounds
As a result, group 2 metals have stronger metallic bonding, which leads to increased cohesive energy and compact atom packing. This explains why group 2 metals are harder and have higher melting and boiling temperatures than group 1 metals.
To learn more about Group 2A(2) refer the link:
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