1,1,2 & single replacement reaction
The heat of the water is shared with the ice and there for you drink will get cold but your ice will melt away from the heat going in the ice
Metallic bonding
The particles in a metal are held together by metallic bonds.
High melting and boiling points
Metallic bonds are strong and a lot of energy is needed to break them. This is why metals have high melting points and boiling points.
Conducting electricity
Metals contain electrons that are free to move in the metal structure, carrying charge from place to place and allowing metals to conduct electricity well.
Metallic bonding - Higher tier
Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalised electrons.
Answer:
Molality = 0.43 m
Explanation:
Given data:
Mass of barium sulfide = 25.4 g
Mass of water = 349 g (349 g/1000 = 0.349 Kg)
Molality of water = ?
Solution:
Number of moles of barium sulfide:
Number of moles = mass/molar mass
Number of moles = 25.4 g/169.39 g/mol
Number of moles = 0.15 mol
Molality:
Molality = number of moles o f solute/ Kg of solvent
Molality = 0.15 mol / 0.349 Kg
Molality = 0.43 m
Answer and Explanation:
<u><em>How are ionic bonds formed?</em></u>
- Ionic bonds are formed as a result of a redox reaction.
- <em>Formation of cations:</em> In which atoms of an element (metal) with low ionization energy give some electrons to reach stable electronic configuration.
- <em>Formation of anions:</em> in which atoms of another element with high electron affinity accepts electrons to achieve a stable electronic configuration.
- <em>Example: NaCl</em>, the sodium atoms loss electron forming Na⁺ and the chlorine atoms gain electron forming Cl⁻, then the ions are attracted to each other with 1:1 ration forming the ionic compound NaCl.
Na + Cl → Na⁺ + Cl⁻ → NaCl
<u><em>What is the attractive force within the ionic bond?</em></u>
- The attractive force within the ionic bond is the electrostatic attraction between the positively charged ions (cations, Na⁺) and the negatively charged ions (anions, Cl⁻).
<u><em> </em></u>
