<span>The atoms in a compound are held together by a chemical bond. The chemical bonds can be either covalent bonds or ionic bonds. Both the bonds are considered very strong bonds. These bonds are mainly formed by sharing of electrons or in the case when one of the elements making the compound donates electron to the other element. The nucleus of each atom attracts to form a strong bond. This property of attraction between the nucleus of the atoms actually helps in forming the chemical bonds. </span>
Answer:
Q = -14322.77 J
Explanation:
Given data:
Mass of water = 55.0 g
Initial temperature = 87.3°C
Final temperature = 25.0 °C
Heat given off = ?
Solution:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Specific heat capacity of water is 4.18 J/g.°C
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = 25.0 °C - 87.3°C
ΔT = - 62.3 °C
Q = 55.0 g×4.18 J/g.°C × - 62.3 °C
Q = -14322.77 J
(3) loses one electron and becomes positively charged
Lithium has one valence electron and Bromine has seven. Therefore Lithium will give up its one to Bromine for both to have an octet
Ionic substances produce ions in solution while molecular substances produce molecules in solution.
<h3>What is a solution?</h3>
A solution is a combination of solute and solvent. The species that occur in solution depends on the type of substance that was dissolved. Since the table is not shown, we do not know exactly what compounds were dissolved in solution.
Generally, if an ionic substance is dissolved in solutions that ions are present in the solution. If a molecular substance is dissolved in solution, molecules are present in solution.
Learn more about solution: brainly.com/question/7932885
Answer:
1. Balanced
2. Unbalanced
3. Unbalanced
Explanation:
<em>Identify which of the following oxidation-reduction reactions are balanced and which are unbalanced in both mass and charge.
</em>
<em>
</em>
<em>1. Ag⁺(aq) + Li(s) → Ag(s) + Li⁺(aq)
</em>
This reaction is balanced in both mass and charge.
<em>2. Fe(s) + Na⁺(aq) → Fe²⁺(aq) + Na(s)
</em>
This reaction is balanced in mass but unbalanced in charge since the charge to the left is +1 and the charge to the right is 2+.
<em>3. K(s) + H₂O(l) → KOH(aq) + H₂(g)</em>
This reaction is balanced in charge but unbalanced in mass since there are 2 atoms of H to the left and 3 atoms of H to the right.
