1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Illusion [34]
1 year ago
8

How the molecule’s properties affect the physical properties of a molecule

Chemistry
1 answer:
Lilit [14]1 year ago
8 0

The intermolecular forces, such as hydrogen bonds or van der Waals attractions, which draw one molecule to its neighbors, govern a substance's physical properties. Due to the relatively weak intermolecular forces of attraction, molecular substances typically take the form of gases, liquids, or low melting point solids.

<h3>How do the intermolecular forces affect physical properties?</h3>

The forces that bind two molecules together are known as intermolecular forces. Intermolecular forces have an impact on physical properties. Strong and weak forces both exist; the stronger the force, the more energy is needed to separate the molecules from one another. As intermolecular forces increase melting, boiling, and freezing points rise.

The following intermolecular forces are listed in order of strength:

  • Van der Waals dispersion forces
  • Van der Waals dipole-dipole interactions
  • Hydrogen bonding
  • Ionic bonds

It would take very little energy to separate two molecules if they are connected by van der Waals dispersion forces. On the other hand, it requires a lot more energy to separate two molecules that are joined together by ionic bonds.

To know more about molecules refer to: brainly.com/question/1819972

#SPJ1

You might be interested in
Challenge question: This question is worth 6 points. As you saw in problem 9 we can have species bound to a central metal ion. T
GenaCL600 [577]

Answer:

CN^- is a strong field ligand

Explanation:

The complex, hexacyanoferrate II is an Fe^2+ specie. Fe^2+ is a d^6 specie. It may exist as high spin (paramagnetic) or low spin (diamagnetic) depending on the ligand. The energy of the d-orbitals become nondegenerate upon approach of a ligand. The extent of separation of the two orbitals and the energy between them is defined as the magnitude of crystal field splitting (∆o).

Ligands that cause a large crystal field splitting such as CN^- are called strong field ligands. They lead to the formation of diamagnetic species. Strong field ligands occur towards the end of the spectrochemical series of ligands.

Hence the complex, Fe(CN)6 4− is diamagnetic because the cyanide ion is a strong field ligand that causes the six d-electrons present to pair up in a low spin arrangement.

5 0
3 years ago
Water is an example of a compound. Which of the following is the best description of all compounds?
AlexFokin [52]

Answer:

A compound has atoms of different elements chemically joined together They can't be separated without a chemical reaction.

3 0
2 years ago
Find the mass of a 60 ML volume of water if the density of water is 1 g/mL
valkas [14]

Answer:  60 grams

Explanation:  (60 ml)*(1g/ml) = 60g

3 0
2 years ago
How is a covalent bond different from an ionic bond?
Alex17521 [72]
A covalent bond is a form of chemical bonding between two non-metals, whereas ionic bonding is a bond between a metal and a non-metal.
8 0
2 years ago
An element with an electronegativity of 0.9 bonds with an element with an electronegativity of 3.1.. Which phase best describes
eduard
Electronegativity is the strength an atom has to attract a bonding pair of electrons to itself. When a chlorine atom covalently bonds to another chlorine atom, the shared electron pair is shared equally. The electron density that comprises the covalent bond is located halfway between the two atoms.

But what happens when the two atoms involved in a bond aren’t the same? The two positively charged nuclei have different attractive forces; they “pull” on the electron pair to different degrees. The end result is that the electron pair is shifted toward one atom.

ATTRACTING ELECTRONS: ELECTRONEGATIVITIES

The larger the value of the electronegativity, the greater the atom’s strength to attract a bonding pair of electrons. The following figure shows the electronegativity values of the various elements below each element symbol on the periodic table. With a few exceptions, the electronegativities increase, from left to right, in a period, and decrease, from top to bottom, in a family.

Electronegativities give information about what will happen to the bonding pair of electrons when two atoms bond. A bond in which the electron pair is equally shared is called a nonpolar covalent bond. You have a nonpolar covalent bond anytime the two atoms involved in the bond are the same or anytime the difference in the electronegativities of the atoms involved in the bond is very small.



Now consider hydrogen chloride (HCl). Hydrogen has an electronegativity of 2.1, and chlorine has an electronegativity of 3.0. The electron pair that is bonding HCl together shifts toward the chlorine atom because it has a larger electronegativity value.

A bond in which the electron pair is shifted toward one atom is called a polar covalent bond. The atom that more strongly attracts the bonding electron pair is slightly more negative, while the other atom is slightly more positive. The larger the difference in the electronegativities, the more negative and positive the atoms become.

Now look at a case in which the two atoms have extremely different electronegativities — sodium chloride (NaCl). Sodium chloride is ionically bonded. An electron has transferred from sodium to chlorine. Sodium has an electronegativity of 1.0, and chlorine has an electronegativity of 3.0.

That’s an electronegativity difference of 2.0 (3.0 – 1.0), making the bond between the two atoms very, very polar. In fact, the electronegativity difference provides another way of predicting the kind of bond that will form between two elements, as indicated in the following table.

Electronegativity DifferenceType of Bond Formed0.0 to 0.2nonpolar covalent0.3 to 1.4polar covalent> 1.5ionic

The presence of a polar covalent bond in a molecule can
Divide
3 0
3 years ago
Other questions:
  • Consider the standard galvanic cell based on the following half-reactions The electrodes in this cell are and . Does the cell po
    15·1 answer
  • How many microliters of original sample are required to produce a final dilution of 10-2 in a total volume of 0.2 mL? 1 microlit
    13·1 answer
  • Which of the following substances would best be measured using mole quantities?
    10·1 answer
  • Heat energy caused by friction is usually a waste product that results when energy
    14·1 answer
  • What does algebra mean
    11·1 answer
  • how long would it take to administer exactly 500 mL of fluid through an IV with a drop factor of 30 gtt/mL if the drip rate is 6
    10·1 answer
  • What is the mass of strontiums isotopes
    6·1 answer
  • 4. The [H+] in solution is 1.0 X 10-3 M. This solution is BEST classified as?
    7·2 answers
  • HURRRY ASAP!!
    10·1 answer
  • Complete the calculation to find the mass of 1 mole of water (H2O). Use the atomic weights given in the periodic table. Select t
    13·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!