Biologists study living things, whereas chemists study nonliving things
Biology has a hierarchy of structural levels, whereas chemistry does not
Chemists study molecules, whereas biologists do not
Chemical systems have emergent properties; biological systems do not
There is no clear distinction because the two sciences are parts of the same whole
H H I I H-O-C-C=O I H
H H I I H-C-H-C=O I H
O I H-N-H
Nonpolar covalent bond
Polar covalent bond
They are isomers.
They are polymers.
They are isotopes
They are ions.
They are both radioactive.
They all have the same number of valence electrons.
Each element exists only in one isotopic form.
They are equal in electronegativity.
They are elements produced only by living cells.
They all have unpaired electrons in their valence shells,
They form ionic bonds in aqueous solutions.
They form covalent bonds in aqueous solutions.
They are stable and unreactive
They exhibit similar chemical behaviors
Both C and D are correct.
Only A and B are correct.
A, B, and C are correct.
Reactions continue with no effect on the concentrations of reactants and products.
Concentrations of products are high.
Reactions have stopped.
Reactions stop only when all reactants have been converted to products.
There are equal concentrations of reactants and products.
Concentration of H+ is 10 times greater than what it was at pH 8.
Concentration of H+ is 100 times less than what it was at pH 8.
Concentration of OH- is 10 times greater than what it was at pH 8.
Concentration of OH- is 100 times greater than what it was at pH 8.
Concentration of H+ is greater and the concentration of OH- is less than at pH 8.
Nonpolar covalent bonds
Polar covalent bonds
Both C and D are correct.
A decrease in the concentration of H2CO3 and an increase in the concentration of HCO3-.
The concentration of hydroxide ion (OH-) to increase.
The concentration of bicarbonate ion (HCO3-) to increase.
The HCO3- to act as a base and remove excess H+ with the formation of H2CO3.
The HCO3- to act as an acid and remove excess H= with the formation of H2CO3.
Molecule collisions in the drink increase.
Kinetic energy in the drink decreases.
A kilocalorie of heat is transferred to the water.
A kilocalorie of heat is transferred to the ice.
Exaporation of the water increases.
H2CO3 is a weak acid, and NaOH is a weak base
H2CO3 is a strong acid, and NaOH is a strong base.
NH3 is a weak base and, and H2CO3 is a strong acid.
NH3 is a strong base, and HCl is a weak acid.
NH3 is a weak base, and HCl is a strong acid.
Releasing H+ in acidic solutions.
Releasing H+ in basic solutions.
Releasing OH- in basic solutions.
Combining with OH- in acidicsolutions.
Combining with H+ in basic solutions.
Small size of the water molecules.
High specific heat of oxygen and hydrogen atoms.
Absorption and release of heat when hydrogen bonds break and form.
Fact that water is a poor heat conductor.
Inability of water to dissapate heat into dry air.