Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

In the structure of ice, cach oxygen atom is surrounded by four other oxygen atoms. (1) tetrahedrally (2) octahedrally (3) square planar manner (4) nonc of these

Short Answer

Expert verified
Option (1) tetrahedrally

Step by step solution

01

Understand the Structure of Ice

Study the arrangement of molecules in the ice structure. Ice has a crystalline structure where each oxygen atom forms hydrogen bonds with four neighboring oxygen atoms.
02

Identify the Geometrical Arrangement

Analyze the geometrical arrangement formed by the oxygen atoms around a central oxygen atom. The bonds are situated at the corners of a tetrahedron.
03

Compare with Given Options

Compare the described geometric arrangement with the given options: tetrahedrally, octahedrally, square planar manner, and none of these.
04

Select the Correct Option

Conclude that the arrangement where each oxygen atom is surrounded by four others in the ice structure is tetrahedral.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

hydrogen bonding in ice
Hydrogen bonding plays a crucial role in the structure of ice. In an ice crystal, each water molecule connects to four adjacent water molecules through hydrogen bonds. This bonding occurs because the hydrogen atoms of one water molecule are attracted to the oxygen atoms of other water molecules.

Imagine water molecules as tiny magnets. The positive (hydrogen) side of one molecule attracts the negative (oxygen) side of another, forming a bond. These bonds are relatively weak compared to covalent bonds but are strong enough to hold the molecules in a specific arrangement.

What's fascinating is that these hydrogen bonds arrange themselves in a way that maximizes distance between each molecule, leading to a less dense structure compared to liquid water. This is why ice floats on water. Unlike in liquids where the molecules are closer together, the hydrogen bonds in ice keep the water molecules spaced apart, making ice less dense.
crystalline structure of ice
Ice has a distinctive crystalline structure that can be visualized as a repeating pattern of water molecules. In this arrangement, every water molecule forms hydrogen bonds with four neighboring molecules, creating a definite pattern.

Think of it like a 3D puzzle where each piece perfectly fits only in a specific orientation. This repeating pattern contains all the water molecules evenly spaced and arranged in layers. Each layer contains hexagonal patterns forming what's known as a hexagonal crystal lattice.

The unique crystalline structure also contributes to the properties of ice, such as its rigidity and its beautiful, symmetrical snowflakes. Snowflakes form when water vapor condenses directly into ice and adopts the hexagonal pattern. This is how we get the stunning and intricate designs we often see.
tetrahedral arrangement
In the ice crystal structure, each oxygen atom is surrounded tetrahedrally by four other oxygen atoms. This means the bonds form a shape resembling a pyramid with a triangular base, known as a tetrahedron.

Visualize a central oxygen atom with four oxygen atoms placed around it at equal distances, positioned at the corners of a tetrahedron. The bond angles forming this arrangement are approximately 109.5 degrees. This specific arrangement is significant because it allows the formation of stable hydrogen bonds.

The tetrahedral arrangement not only affects the microscopic structure but also explains many of ice's macroscopic properties, like its density and melting behavior. For instance, as ice melts, this tetrahedral arrangement breaks down, allowing water molecules to get closer together, explaining why liquid water is denser than ice.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following statement is false? (1) Hydrogen can be placed in the halogen group because it forms hydrides like chlorides. (2) The best explanation for not placing hydrogen with the group of alkali metals or halogens is that the IP of \(\mathrm{H}_{2}\) is too higher than alkali metal but too low than halogens. (3) The tendency of hydrogen to gain one electron to acquire He configuration resembles halogens. (4) Hydrogen molecules are diatomic and form \(\mathrm{H}\) ions similar to halogens.

Which of the following statements regarding saline hydridcs is falsc? (1) Saline hydrides are formed only by thosc clements which have very low electronegativity values and can transfer clectrons to the hydrogen atom. (2) Salt-like hydrides are solids with ionic lattices. (3) In fused state, saline hydrides conduct electricity. (4) The density of salt-like hydrides is lesser than the parent metal.

Partial hydrolysis of one mole of peroxydisulphuric acid produces (1) Two moles of sulphuric acid (2) Two moles of peroxy monosulphuric acid (3) One mole of sulphuric acid and one mole of peroxy monosulphuric acid (4) Two moles of sulphuric acid and one mole of hydrogen peroxide

Commercial hydrogen is obtained from (1) coal gas (2) water gas (3) air (4) producer gas

The wrong statement among the following is (1) Ionic hydrides are formed by clements of high electropositive character. (2) Phosphinc is an cxamplc of clectron-prccise hydridc. (3) Titanium hydride is a metallic hydride. (4) Mctallic hydrides on reacting with water give hydrogen.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free