The equal mass indicates that both atoms have the same number of protons and neutrons.
A positive charge signifies a difference in electron count.
Assuming the atomic number is A,
the mass number equals M.
In a neutral atom, there are A electrons.
A negatively charged atom would have A + 1 electrons [while the count of protons and mass number remains unchanged].
A positively charged atom contains A - 1 electrons [with consistent protons and mass number].
For instance: Cl- and Cl+.
Answer:
Calcium's atomic radius is roughly 175 pm.
Explanation:
We know that magnesium has an atomic radius of 150 pm.
The atomic radius of strontium measures 200 pm.
Since calcium's position is between magnesium and strontium in group 2 of the periodic table, its atomic radius should be roughly averaged between magnesium's and strontium's atomic radii because atomic radius is not constant.
Thus;
Calcium's atomic radius is approximately calculated as follows;
The average atomic radius is (200 + 150)/2 = 175 pm.
Response:
9.606 g
Clarification:
Step 1: Write the balanced combustion equation
C₂H₆O(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(g)
Step 2: Determine the moles for 11.27 g of H₂O
The molar mass of H₂O is 18.02 g/mol.
11.27 g × (1 mol/18.02 g) = 0.6254 mol
Step 3: Find the moles of C₂H₆O that produced 0.6254 moles of H₂O
The ratio of C₂H₆O to H₂O is 1:3. Thus, the moles of C₂H₆O are 1/3 × 0.6254 mol = 0.2085 mol
Step 4: Calculate the mass for 0.2085 moles of C₂H₆O
The molar mass of C₂H₆O is 46.07 g/mol.
0.2085 mol × 46.07 g/mol = 9.606 g
E = mc²
where E = energy produced
m = mass of the nucleus
C = speed of light
m = 9.106 x 10⁻³ x 1.67 x 10⁻²⁷ kg
C = 3 x 10⁸ m/s, thus C² = 9 x 10¹⁶
E = 1.37 x 10⁻¹² J
(c) Cu + S → CuS is classified as a redox reaction
Explanation:
The following reactions are presented:
(a) K₂CrO₄ + BaCl₂ → BaCrO₄ + 2 KCl
(b) Pb²⁺ + 2 Br⁻ → PbBr₂
(c) Cu + S → CuS
Reaction (c) represents a redox reaction, as the oxidation states of the elements are changing. In this case:
Cu + S → CuS
In its elemental form, Cu has an oxidation state of 0, while in CuS (copper sulfide), its oxidation state changes to +2.
Similarly, S in its elemental form has an oxidation state of 0 and is -2 in CuS (copper sulfide).
Learn more about:
redox reactions
