Answer:In ionic compounds, electrons are transferred between atoms of different elements to form ions. But this is not the only way that compounds can be formed. Atoms can also make chemical bonds by sharing electrons equally between each other. Such bonds are called covalent bonds. Covalent bonds are formed between two atoms when both have similar tendencies to attract electrons to themselves (i.e., when both atoms have identical or fairly similar ionization energies and electron affinities). For example, two hydrogen atoms bond covalently to form an H2 molecule; each hydrogen atom in the H2 molecule has two electrons stabilizing it, giving each atom the same number of valence electrons as the noble gas He.
Compounds that contain covalent bonds exhibit different physical properties than ionic compounds. Because the attraction between molecules, which are electrically neutral, is weaker than that between electrically charged ions, covalent compounds generally have much lower melting and boiling points than ionic compounds. In fact, many covalent compounds are liquids or gases at room temperature, and, in their solid states, they are typically much softer than ionic solids. Furthermore, whereas ionic compounds are good conductors of electricity when dissolved in water, most covalent compounds are insoluble in water; since they are electrically neutral, they are poor conductors of electricity in any state.
Answer:
The increase of prey
Explanation:
Without predators in the ecosysten prey population would increase
Answer:
P= 7.01 atm
P(CO₂)= 2.34 atm
Explanation:
Step 1: Convert the temperature to Kelvin
We will use the following expression.
K = °C + 273.15
K = 32.0°C + 273.15 = 305.2 K
Step 2: Calculate the total number of moles of the mixture
We will use the following expression.
n = nCO₂ + nN₂ = 2.33 mol + 4.66 mol = 6.99 mol
Step 3: Calculate the total pressure of the mixture
We will use the ideal gas equation.
P × V = n × R × T
P = n × R × T / V
P = 6.99 mol × 0.0821 atm.L/mol.K × 305.2 K / 25.0 L
P= 7.01 atm
Step 4: Calculate the partial pressure of carbon dioxide
We will use the ideal gas equation.
P(CO₂) × V = nCO₂ × R × T
P(CO₂) = nCO₂ × R × T / V
P(CO₂) = 2.33 mol × 0.0821 atm.L/mol.K × 305.2 K / 25.0 L
P(CO₂)= 2.34 atm
