entities that are self replicating, capture energy from their environment, and adapt to changes in their environment
If something is alive it can
E) All of these answers
Are crystals considered alive? Why or why not?
No. They grow but cannot adapt.
True or False: Living organisms have adapted to all of the following conditions:
•High salt environments
•Cold environments
•Ice
•High sulfur environments
•High temperature
•Low oxygen
•No oxygen
True
Name for basic building blocks of life.
1) Sugars
2) Carbohydrates
3) Lipids
4) Proteins
What is typically used for the transfer of energy in cells?
C) ATP
True or False: Living systems are studied at many levels including nonliving atoms and small molecules.
True. Nonliving atoms and small molecules are covered in chapter 1 of our book.
True of False: Six atoms out of the entire periodic table make up approximately 98 percent of the mass of all living systems.
True
Which six atoms make up approximately 98 percent of the mass of all living systems?
1) Hydrogen (H)
2) Carbon (C)
3) Nitrogen (N)
4) Oxygen (O)
5) Phosphorus (P)
6) Sulfur (S)
True or False: The major atomic components of living systems are major components of the Earths Crust.
False
True or False: H, C, N, O, P, and S are the atomic components of sugars, carbohydrates, proteins, lipids, and nucleic acids.
True
The nucleus of an atom
B) has a positive charge caused by the protons
Protons have a charge of
A) 1.60 x 10-19 Coulombs
Electrons have a charge of
D) -1.60 x 10-19 Coulombs
Protons and neutrons have
D) the same mass
Protons and electrons
A) have different charges of the same magintude
The mass of a proton or neutron is
C) 1.67 x 10-24 g
True or false: Electrons have a mass which is considered negligible compared to protons and neutrons.
True. Their mass is 9.1 x 10-28 g
True or False: The electron cloud is the most dense part of an atom.
False. The nucleus is the most dense part of an atom.
True or False: In order to balance charge in an atom, there needs to be significantly more electrons to compensate for the larger protons.
False. Number of protons = number of electrons in an atom to balance charge. They have opposite charges of the same magnitude.
Define Element
Each of more than one hundred substances that cannot be chemically interconverted or broken down into simpler substances and are primary constituents of matter. Each element is distinguished by its atomic number, i.e., the number of protons in the nuclei of its atoms.
Define Atomic Number
The number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table.
Define Atomic Mass
The mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes.
Define Isotope
Each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties; in particular, a radioactive form of an element.
Define Mol
The base unit of amount of pure substance in the International System of Units that contains the same number of elementary entities as there are atoms in exactly 12 grams of the isotope carbon 12.
6.02 x 1023 atoms
True or False: Energy changes constantly in an electron orbital.
False. Energy is constant in an electron orbital
Larger orbitals have
B) higher energy
True or False: For all elements, electrons fill in the lowest energy electron orbitals first. The outermost orbital may be partially full.
True
Valence is
D) the number of electrons in the outermost shell
True or False: Protons are responsible for the combining capacity of the atoms (ionic and covalent bonds).
False. Valence electrons are responsible for the combining capacity of the atoms (ionic and covalent bonds).
How many valence electrons does hydrogen have?
A) 1
How many valence electrons does carbon have?
B) 4
How many valence electrons does nitrogen have?
B) 5
How many valence electrons does oxygen have?
C) 6
How many valence electrons does phosphorous have?
D) 5
How many valence electrons does sulfur have?
C) 6
True or False: A covalent bond forms when two orbitals each containing 1 electron merge due to the attraction of the electrons to the protons
True. They share electrons.
Define Molecule
The smallest possible amount of a particular substance that has all the characteristics of that substance. 2 or more atoms bonded together.
What freedom does a molecule lose when it has a double bond as opposed to a single bond?
The freedom to rotate.
True or False: Triple bonds are highly common in biological systems.
False.
Which covalent bond requires the most energy to break?
D) C==O
Which covalent bond requires the least energy to break?
B) N--O
True or False: The bond between the hydrogen atoms and the carbon atom in H2O is an example of a polar covalent bond.
True.
Cations are
B) ions with a positive charge
Anions are
C) ions with a negative charge
Define Hydrogen Bond
An electrostatic attraction between a hydrogen atom in one polar molecule (as of water) and a small electronegative atom (as of oxygen, nitrogen, or fluorine) in usually another molecule of the same or a different polar substance
Describe the effect of van der Waals forces in water.
Water molecules in liquid water are attracted to each other by electrostatic forces
What is the pH of water at 25 degrees celsius?
B) 7
True or False: Enzymes increase the activation energy of a reaction.
