Unit 1 (all cards) Flashcards
Define anatomy
Examining the structure of the human body
Define physiology
The study of function of the human body
True or false: Anatomy and physiology complement each other; you can not entirely separate the two because of the unity of form and function
True
Define gross anatomy
Study of structures that can be seen with the eyes
What are three examples of gross anatomy being applied in medicine?
Dissection, exploratory surgery, and medical imaging
Name 3 areas that study anatomical structures too small to be seen with the naked eye
Histology, cytology, and ultrastructure
What is another name for histology?
Microscopic anatomy
What is histology?
The examination of tissues [under a microscope]
What is cytology?
The study of structure and function of cells
What is ultrastructure?
Viewing detail under an electron microscope
Name 3 subdisciplines of physiology
Neurophysiology (physiology of the nervous system)
Endocrinology (physiology of hormones)
Pathophysiology (mechanisms of disease)
Define pathophysiology
The study of mechanisms of disease
Define comparative physiology
The study of another species to learn about body functions
What is the basis for much of our understanding of human physiology and the development of new drugs and medical procedures?
Comparative physiology
Why is comparative physiology important to research in physiology as a whole?
Physiology, unlike anatomy, requires live subjects due to the fact that you cannot observe function on a cadaver, so often relies on animals to perform research
Define organization in anatomy
The idea that living things exhibit a higher level of organization than nonliving things.
Living matter is always compartmentalized into ____ or more cells.
one
What is cellular composition?
The idea that living matter is always compartmentalized into one or more cells.
What is metabolism?
Internal chemical reactions
True or false: all chemical reactions that take place inside your body are considered to be a part of your metabolism
True
Define responsiveness in biology
The ability to sense and react to stimulate (irritability or excitability).
Define movement in biology
The movement of organisms and/or of substances within the organism.
Define homeostasis
Maintaining relatively stable internal conditions (regardless of external conditions)
What is the one word that can sum up many of the topics covered in A&P one and two?
Homeostasis
Define development in biology
Differentiation and growth
Differentiation and growth make up the concept of ________.
development.
Give an example of why monitoring development is important to medicine
Looking a developing fetus in the womb to see if structures are differentiating and growing at the typical rates.
Define reproduction
Producing copies of themselves; passing genes to offspring.
Define evolution in biology
Changes in genes at the population level
Give an example of evolution that is relevant to modern medicine
Bacteria evolving to resist antibiotics on a population level.
What is the general idea of the body’s structural hierarchy of complexity?
Atoms are the least complex component of life, organisms are the most complex.
Define elements
The simplest form of matter with unique properties.
All elements are made up of what three things?
Electrons, protons, and neutrons
What are the three main elements covered in this course?
carbon, oxygen, and nitrogen
Define atomic number
The number of protons in an element; this gives the element its identity
Define protons
A positively charged particle within atoms, the number of which give the atom its elemental identity
What two things are located in the nucleus of an atom?
Protons and neutrons
Where are electrons located?
Around the nucleus
What is atomic mass?
Number of protons + number of neutrons = atomic mass
Define an isotope
Atoms with a missing or extra neutron
Define a neutron
A neutral particle in the nucleus of an atom that gives the element its atomic mass
Define an electron
A small negatively charged particle that orbits the nucleus of an atom
The first energy shell is full with _ electrons, the second shell is full/ stable with _ electrons, and the third shell is full/stable with _ electrons.
The first energy shell is full with 2 electrons, the second shell is full/ stable with 8 electrons, and the third shell is full/stable with 8 electrons.
Ionization occurs because _____
atoms want their shells to be stable and full of electrons.
Define an ion
A substance that has a charge from gaining or losing electrons
Define cation and anion
Cation: positively charged ion
Anion: negatively charged ion
Define ionic bond
A charge attraction between a cation and anion.
Define valence electrons
Electrons in the outermost shell
What is a covalent bond and how is it represented?
A bond through shared valence (outer) electrons. Usually represented by a dash or subscript (i.e. H-H or H₂)
Like a ____, water molecules have charged regions
battery
What kind of bond is found in water molecules?
Polar covalent bonds
Define polar versus nonpolar
Polar = evenly shared electrons Nonpolar = unevenly shared electrons
What are polar covalent bonds?
Electrons are shared unequally within a covalent bond.
Give an example of an nonpolar molecule
O^2
Which of the following repel each other and don’t mix?
a) polar and polar bonds
b) polar and nonpolar bonds
c) nonpolar and nonpolar bonds
b) polar and nonpolar bonds
Why don’t oil and water mix?
Because nonpolar and polar bonds hate each other; lipids found in oil are mostly made of nonpolar covalent bonds, and water has polar covalent bonds.
Define hydrogen bonds
The weakest type of bond formed because of attraction between a slightly positive hydrogen and a slightly negative oxygen (or nitrogen).
What is the weakest type of bond?
Hydrogen bonds
When you put two molecules of water together, they form a hydrogen bond. Why?
The polar covalent bonds allow for the hydrogen bonds between water molecules.
Define cohesion and adhesion
Cohesion: Water is attracted to water
Adhesion: Water is attracted to other substances.
What mixes in water?
Substances similar to water (meaning polar, charged ions).
Define a solution in chemistry
A mixture of dissolved substances called solutes, and dissolving agents called solvents.
What is the most common solvent used in this class? Why?
Water, because our bodies are mostly water
Define a mixture
A combination of two or more elements without a chemical reaction
What are the four types of organic molecules?
Proteins, lipids, carbohydrates, and nucleic acids
What are the monomers and polymers of proteins?
Monomers = amino acids Polymers = polypeptides
Where did polypeptides get their name?
The bond between amino acids is called a peptide bond
What are the monomers and polymers of carbohydrates?
Monomers = monosaccharides Polymers = Polysaccharides, starch, glycogen, cellulose
What are the monomers and polymers of lipids?
Monomers = for triglycerides: glycerol, 3 fatty acids Polymers = phospholipids
What are the monomers and polymers of nucleic acids?
Monomers = Nucleotides Polymers = DNA, RNA, ATP
Proteins: There are ____ amino acids
20
Proteins: Side chains (also called the R group) can be _____ or _____.
Polar or nonpolar
Proteins: What do side chains/ the R group determine?
They can be polar or nonpolar, which determines how amino acids interact with each other.
Proteins: The sequences of amino acids determine what?
How the protein folds, which determines the protein’s function.
What are the four structures of proteins?
Primary structure = amino acid sequence
Secondary structure = hydrogen bonding between amino acids
Tertiary structure = interactions of side chains
This is what makes each protein really unique.
Quaternary structure = two or more polypeptides
In proteins, shape determines ______.
function
The hydrogen of one water molecule is attracted to what part of the other water molecule?
The negative part
What does it mean when we say that water is polar?
It means that water shares its electrons unequally between the oxygen atom and the hydrogen atom, which creates charge regions, which creates a partial charge.
The attraction between parts of two different polar molecules is called ______ bonding.
hydrogen
True or false: Hydrogen bonding usually takes place between two of the same molecule.
False; hydrogen bonding usually takes place between two different molecules (usually a molecule with hydrogen + one with oxygen or a molecule with hydrogen + one with nitrogen)
The tendency for molecules of water to cling to one another, is that an example of adhesion or cohesion?
Cohesion
Give an example of why cohesion (water sticking to water) is important to the human body
The water on the surfaces of our lungs clings to the water on the surface of our inner chest muscles, which is what allows our lungs to inflate when our chests rise (if the cohesion is lost, lungs can collapse).
Why does water bead up on some substances and soak into others?
Because some substances, like wax paper (which consists of lipids), have primarily non-polar bonds, which repel oxygen’s polar covalent bonds.
Why do we use cotton towels to dry ourselves when we get out of the shower?
Because cotton has a polar charge, which allows it to bind to water and dry you
Non-polar bonds of a substance (like oil or soap) repelling the polar bonds of water can lead to what?
Decreased surface tension
Why can insects walk on water?
Surface tension
Will nonpolar and polar molecules interact?
No
What happens when you bring two chloride ions together?
They repel each other because they are both negatively charged
Which of the following would have a higher level of salt: A solution of 15% NaCI or a solution of 30% NaCI?
30% NaCI
Which of the following would have a higher level of water: A solution of 15% NaCI or a solution of 30% NaCI?
15% NaCI
In a solution of 15% NaCI, is water the solute or solvent? What about the NaCI?
Water is the solvent and NaCl is the solute
What four types of molecules mix with water?
Polar molecules, hydrophilic molecules, molecules with ionic bonds, and proteins (most contain polar covalent bonds; some are anions)
What two types of molecules don’t mix with water?
Nonpolar and hydrophobic molecules
In the human body, nutrients, including vitamins, are transported to the cells by the blood. Vitamins can be divided into two types– water-soluble vitamins and fat-soluble vitamins. Since blood is mostly water, the water-soluble vitamins are easily transported to their destinations. How do you think the fat-soluble vitamins travel in the blood?
Proteins pick them up and carry them.
Define elements
The simplest form of matter to have unique chemical properties cannot be broken down by ordinary chemical means
How many naturally occurring elements are there?
91
Define atoms
The building blocks for each element
How many elements have a biological role?
24
What 6 elements make up 98.5% of our body weight?
Oxygen (O) Carbon (C) Hydrogen (H) Nitrogen (N) Calcium (Ca) Phosphorus (P
Lesser elements make up what percent of the body?
0.8%
Trace elements make up what percent of the body?
Less than 0.7%
Where and in what quantity are trace elements found in the body?
They’re required in minute amounts and are found as a part of enzymes
Give examples of lesser and trace elements
Lesser: K, S, Na, Cl, Fe, Mg
Trace: I, Co, Cu, Z, Cr, etc.
Define minerals
Inorganic elements extracted from soil by plants and passed to humans
What percent of our body weight is made up of minerals?
4%
What two minerals are most commonly found in the body? What are some other minerals in the body?
Mostly Ca and P (also Cl, Mg, K, Na, and S)
Define electrolytes in the context of minerals
Mineral salts needed for nerve and muscle function
What are the three components of atoms?
Protons, neutrons, and electrons
This is just a note to myself that this chapter does also cover the basics of protons, neutrons, and electrons, but those flashcards can be found in lab 2
Elements with an abnormal number of neutrons are called ____
Isotopes
Average of mass numbers of an element = ______
Atomic weight
True or false: most isotopes are stable. Why?
True; few will disintegrate and give off energy
Intense radiation can be ionizing, how does this affect the body?
Intense radiation can be ionizing (ejects electrons, destroys molecules) and can cause genetic mutations and cancer
Where are radioactive isotopes used in medicine? What are some other examples?
Used for radiation therapy and diagnostic procedures. This includes PET scans, using I-131 determine size and activity of the thyroid gland, Hida scans (Tc-99 technetium with a ½ life of 6 hours), Cobalt-60 for cancer
Other examples of radioactive isotopes include UV radiation, X-rays, alpha particles, beta particles, gamma rays
True or false: All elements have at least one radioisotope
True
True or false: X-rays and CT scans use radioactivity
False; they use very short electromagnetic waves.
Electron shells are also called ________
energy levels
In neutral atoms, number of electrons equals number of protons. Non-neutral atoms have a different number of electrons than normal; what are they called?
Ions (or electrolyte)
Define cations and anions
Anion—particle that gains electron(s) (net negative charge)
Cation—particle that loses electron(s) (net positive charge)
Ions with _____ charges are attracted to each other
a) opposite
b) same
a) opposite
Define electrolytes
Substances that ionize in water (acids, bases or salts)
Define salts
A compound (ex: NaCl) that can dissociate into water and contains cations (Na) and anions (Cl)
Define a molecule
Chemical particle composed of two or more atoms united by a chemical bond
Define a compound
Molecule composed of two or more different elements
Define molecular formula
Identifies constituent elements and how many atoms of each are present
Define structural formula
Identifies the location of each atom
What do chemical bonds do?
They hold atoms together within a molecule or attract one molecule to another
What are the three most important types of chemical bonds?
Ionic bonds, covalent bonds, and hydrogen bonds
Inert elements have a ____ outer shell
a) incomplete
b) full
b) full
Reactive elements have a ____ outer shell
a) incomplete
b) full
a) incomplete
Define ionic and covalent bonds
Ionic bonds: will transfer (gain/lose) electrons
Covalent bonds: will share electrons
Describe ionic bonds in detail (the attractions are between ____ and ____; electrons are shared or transferred; how easily are they broken)
Attractions between anions and cations
Electrons donated from one atom to another
Easily broken by water
____ compounds form crystals instead of individual molecules
Ionic
Define a single covalent bond
One pair of electrons is shared
What is the strongest type of bond?
Nonpolar bonds
In what type of bonds do electrons spend more time near oxygen?
Polar bonds
Define polar and nonpolar bonds
Nonpolar bond: electrons shared equally (strongest bond)
Polar bond: electrons shared unequally (spend more time near oxygen)
_____ sharing of electrons produces polar molecules
Unequal
What is an example of an intermolecular hydrogen bond? An intramolecular hydrogen bond?
Intermolecular hydrogen bond between water molecules
Intramolecular hydrogen bonds helps protein folding; holds sides of DNA together
Define hydrogen bonds
Weak charge attraction between a slightly positive hydrogen and a slightly negative oxygen (or nitrogen)
Define mixtures
When elements/molecules/objects are physically blended but not chemically combined
What are body fluids?
Complex mixtures of chemicals
What percent of the body is made up of water? What factors determine this?
Water is 50% to 75% of body weight; this depends on age, sex, fat content, etc.
What two things give water the properties to support life? What are these properties?
Polar covalent bonds and a V-shaped molecule give water solvency, cohesion, adhesion, chemical reactivity, and thermal stability
Define solvency
The ability to dissolve other chemicals
Define hydrophilic and hydrophobic
Substances that dissolve (mix) with water are Hydrophilic
Substances that do not mix easily with water are Hydrophobic
What is the universal solvent?
Water
Metabolic reactions depend on ______ of water
solvency
Define adhesion versus cohesion
Adhesion—water adheres to other substances
Cohesion—water molecules cling to each other
Give an example of adhesion in the body
Water adheres to large membranes reducing friction around organs
Water adhering to large membranes is an example of _____
adhesion
Why is water so cohesive?
Its hydrogen bonds
What is surface film (think bugs walking on water) on the surface of water due to?
Surface film on surface of water is due to molecules being held together by surface tension
Which element’s thermal stability helps stabilize the internal temperature of the body?
Water’s
Define high heat capacity and explain why water’s heat capacity is so high
Something with a high heat capacity absorbs and releases large amounts of heat before changing temperature.
In water, hydrogen bonds inhibit temperature increases by inhibiting molecular motion.
What is an effective coolant?
Water
What is chemical reactivity?
The ability to participate in chemical reactions
Water ionizes into what two things?
H^+ and OH^−
What can water ionize?
Water ionizes many other chemicals (acids and salts)
Define acids
A substance that dissociates in solution to produce hydrogen ions (H+) and anions.
Define bases (also called alkalines)
A substance that dissociates in solution to yield cations and hydroxide ions (OH-).
Name two important bases (aka alkalines) in the body
Bicarbonate ion (HCO3–) and ammonia (NH3) are important bases in the body
Define salt
A substance that dissociates in solution producing cations and anions but not hydrogen ions or hydroxide ions.
Define the three pH categories
Acidic: pH 0–6.99
Basic: pH 7.01–14
Neutral: pH 7.00
Body fluids each have their own ____ range they must maintain.
pH
What can help prevent large changes in pH?
Buffers
Define energy
The capacity to do work [move something]
True or false: all body activities are forms of work
True
Define potential energy and give an example
Energy stored in an object, but not currently doing work (ex: water behind a dam waiting to be released)
Define chemical energy and free energy
Chemical energy—potential energy in molecular bonds
Free energy—potential energy available in a system to do useful work
Define kinetic energy and give an example
Energy of motion, doing work
Example: water flowing through a dam, generating electricity
Define heat
Kinetic energy of molecular motion
Define a chemical reaction
A process in which a covalent or ionic bond is formed or broken
Define chemical equation
Symbolizes the course of a chemical reaction (reactants into products)
What are the two classes of chemical reactions?
Decomposition and synthesis reactions
What are decomposition reactions?
A large molecule breaks down into two or more smaller ones (i.e. AB > A + B)
What are synthesis reactions?
Two or more small molecules combine to form a larger one (i.e. A + B > AB)
Define reversible reactions. When do they reach equilibrium?
Reactions that can go in either direction under different circumstances. They reach equilibrium when ratio of products to reactants is stable.
When do reactions occur?
When molecules collide with enough force and correct orientation
When do reaction rates increase?
When:
the reactants are more concentrated
the temperature rises
a catalyst is present
Define metabolism
All chemical reactions of the body
Define catabolism
Energy-releasing decomposition reactions that break covalent bonds and produce smaller molecules
Define anabolism
Energy-storing synthesis reactions that require energy input and the production of protein or fat
Catabolism and anabolism are inseparably linked. Why?
Anabolism is driven by energy released by catabolism
Define organic chemistry
The study of compounds containing carbon
What are the four categories of carbon compounds/ organic molecules?
Carbohydrates, lipids, proteins, and nucleic acids
Define macromolecules
Very large organic molecules with high molecular weights
Define polymers and give an example
Macromolecules made of a repetitive series of identical or similar subunits (monomers).
Ex: starch is a polymer of about 3,000 glucose monomers.
Monomers are linked together by ____________ and polymers are broken apart by _____
Monomers are linked together by dehydration synthesis and polymers are broken apart by hydrolysis
Define dehydration synthesis
Monomers covalently bind together to form a polymer with the removal of a water molecule
Define hydrolysis
Splitting a polymer by the addition of water
What is the primary function of carbohydrates?
Energy
What is the general formula of carbohydrates? Give an example.
(CH2O)n, n = # of carbon atoms
Ex: glucose, n = 6, so formula is C6H12O6
What are the three sizes of carbohydrate molecules
Monosaccharides, disaccharides, and polysaccharides
What are the three types of monosaccharides? How are they produced?
Glucose, galactose, and fructose. They’re produced by digestion of complex carbohydrates
What is glucose known as in medicine?
Blood sugar
Define isomer
Same molecular formula – different arrangment
What are the three types of disaccharides?
Sucrose, lactose, and maltose
What is sucrose?
A disaccharide known as table sugar
Glucose + fructose
What is lactose?
A disaccharide known as sugar in milk
Glucose + galactose
What is maltose?
A disaccharide known as grain products
Glucose + glucose
Give an example of a polysaccharide
Glycogen
What is glycogen and where is it found in the body?
A glucose polymer that is stored in the liver and skeletal muscles
Define starch
Energy storage in plants in the form of carbohydrates that is digestible by humans
Define cellulose
A structural molecule in plants that’s a carbohydrate that is important for human dietary fiber (but indigestible to us)
Are carbohydrates hydrophilic or hydrophobic?
Simple carbohydrates are small polar molecules (containing several -OH groups) which makes them hydrophilic
Why are lipids only made up of one group?
Because either part of or the entire molecule is hydrophobic.
What makes lipids different from carbs and proteins?
Usually contains more nonpolar covalent bonds than carbs or proteins
True or false: lipids are a very diverse group
True
What is the difference between saturated and unsaturated fatty acids?
Saturated fatty acids have a lot of hydrogen
Unsaturated fatty acids contain some double bonds
Essential fatty acids must be obtained from food
What are triglycerides (neutral fats)?
Three fatty acids linked to glycerol
What is the primary function of triglycerides (neutral fats)? What other thing does it help with?
Their primary function is energy storage (2x more energy than carbs or proteins). They also help with insulation and padding (shock absorption (adipose tissue))
Since triglycerides are hydrophobic, how are they transported in the human body?
Proteins have to carry them (not sure about this one)
What are phospholipids?
They are similar to neutral fats except one fatty acid is replaced by a phosphate group
Phospholipids are made up of a ___ and ____
head and tail
What is the “parent” steroid from which the other steroids are synthesized?
Cholesterol
Give some examples of steroids
Cholesterol, cortisol, progesterone, estrogens, testosterone, and bile acids
What are steroids important for?
They’re important for nervous system function and structural integrity of all cell membranes
15% of our cholesterol comes from our diet, where does the other 85% of cholesterol come from?
85% is internally synthesized (mostly in liver)
Define a protein
A polymer of amino acids
Define amino acids and what three things are attached to it.
They are a central carbon with three attachments:
an amino group (NH2), carboxyl group (—COOH), and a radical group (R group)
What determines the properties of an amino acid?
The R group
How many amino acids are there?
20
Amino acids only differ from each other in what way?
The R groups differ
What is a peptide?
Any molecule composed of two or more amino acids joined by peptide bonds
How are peptides named?
According to the number of amino acids they have: Dipeptides have 2 Tripeptides have 3 Polypeptides many Proteins have more than 50
Peptides are a component of ____
Proteins
How do peptide bonds form?
Dehydration synthesis creates a peptide bond that joins the amino acid of one group to the carboxyl group of the next.
What does the confirmation of a protein mean?
The unique, three-dimensional shape of protein crucial to function
What is crucial to the function of a protein?
Its confirmation
True or false: Proteins can reversibly change conformation and thus function
True
Define denaturation and what causes it. Give an example.
Extreme conformational change that destroys the function of a protein caused by extreme heat or pH.
Example: when you cook an egg
What are three specific examples of body functions that require proteins?
Muscle contraction, enzyme catalysis, and membrane channel opening
What are the four levels of protein structure?
Primary, secondary, tertiary, and quaternary
What are the seven main functions of proteins?
Structure, communication, membrane support, catalysis, recognition & protection, movement, and cell adhesion
Give an example where proteins help with structure
In keratin and collagen.
(Keratin—tough structural protein of hair, nails, skin surface
Collagen—contained in deeper layers of skin, bones, cartilage, and teeth)
Give an example where proteins help with communication
Between some hormones and receptors
Give two examples where proteins help with membrane transport.
Channel proteins in cell membranes govern what passes. Carrier proteins transport solutes to other side of membrane.
Give an example where proteins are needed for catalysis
Most enzymes are globular proteins
Give an example where proteins help with recognition and protection
Antibodies are proteins
Give an example where proteins help with movement
Motor proteins are molecules with the ability to change shape repeatedly
Define motor proteins
Molecules with the ability to change shape repeatedly
Give examples where proteins help with cell adhesion
Proteins bind cells together (example: sperm to egg)
and keep tissues from falling apart
What are enzymes and what do they do for our bodies?
They’re proteins that function as biological catalysts by lowering activation energy. They permit reactions to occur rapidly at body temperature
What permits reactions to occur rapidly at body temp?
Enzymes
Define substrate
A substance an enzyme acts upon
How are enzymes named?
Named for substrate with -ase as the suffix
Amylase enzyme digests starch (amylose)
What are the three steps of an enzymatic reaction?
1) Enzyme and substrate
2) Enzyme-substrate complex
3) Enzyme and reaction products
True or false: enzymes are reusable and not consumed by their reactions
True
Are enzymes fast or slow?
They work at an astonishing speed: One enzyme molecule can consume millions of substrate molecules per minute
What can change enzyme shape and function? What does changing an enzymes function do?
Temperature, pH and other factors can change enzyme shape and function, which can alter ability of enzyme to bind to substrate
Are proteins hydrophilic or hydrophobic?
Hydrophilic
Nucleic acids: Monomers are called _____
nucleotides
Nucleic acids: What are the four components of nucleotides?
1- Nitrogenous base
2- Adenine, Guanine, Cytosine, Thymine or Uracil
3- Sugar (ribose or deoxyribose)
4- One or more phosphate groups
Nucleotides become polymers called nucleic acids; what are three examples of nucleic acids?
ATP, RNA, and DNA
Nucleic acids: Describe DNA
Contains millions of nucleotides
Constitutes genes
Instructions for synthesizing proteins
Nucleic acids: Describe RNA’s function
A nucleic acid that follows DNA instructions to assemble proteins
Nucleic acids: Describe ATPs function
ATP is body’s most important energy-transfer molecule
Holds energy in covalent bonds
Most energy transfers to and from ATP involve adding or removing the third phosphate
Which of the following are examples of compounds? a) O2 and CO2 b) O2 and H2O c) CO2 and H2O d) all of the above Bonus points: Why?
c) CO2 and H2O
Explanation: a compound contains two or more elements, and although O2 is a molecule, it is not a compound because it only has one element
True or false: a proton or electron of Carbon will act the same as a proton or electron of Oxygen.
True
Why do our bodies need iron?
Iron is needed for our blood; oxygen doesn’t go through blood on its own, so iron is needed to grab it and carry it around. This is why we have things like iron infused cereals.
Why do our bodies need iodine?
Iodine is used by the thyroid in thyroid hormones which are used for metabolism; you don’t need a lot, but if you don’t have it, you can’t make those hormones. This leads to low energy, cold feeling, etc. This is why we use iodized salt.
Give an example of why minerals are important to our bodies using potassium
High or low potassium (K) = cardiac arrest
What can radioactive isotopes do that stable isotopes can’t?
They disintegrate and give off energy, and this energy can break chemical bonds
Give an example of using radioactive isotopes to negatively effect the human body
A former spy of soviet union was poisoned by someone putting a radioactive story in his tea (head this story before) and died due to radiation poisoning over a period of weeks.
Give an example of how radioactive isotopes are used in human medicine
We have ways to detect energy (like energy given off by radioactivity) and pick it up on a scan, so we can use these radioactive isotopes to see different parts of the brain (like plaques on the brains of Alzheimer’s pts)
True or false: atoms are not electrically neutral when they’re not ions
False; they are electrically neutral
True or false: you always fill the inner electron shells first
True
Give an example of something that’s a molecule but not a compound, and explain why
O2 is a molecule but not a compound, because compounds have two or more different elements.
Give an example of the importance of structural formula
Shape/location/structure can determine function (ex: glucose, fructose, and galactose all have the same formula, but different properties)
Give an example of inert elements with a full outer shell
Noble gasses
How are single covalent bonds usually represented?
Represented by a solid line
A weak charge attraction is also called a ____ ____
Hydrogen bond
Define intermolecular and intramolecular
Intermolecular: between individual molecules
Intramolecular: within an individual molecule
The intramolecular bonds in water are ____ _____ bonds, the intermolecular bonds between water molecules are _____ bonds
The intramolecular bonds in water are polar covalent bonds, the intermolecular bonds between water molecules are hydrogen bonds
The six most abundant elements in the human body are carbon, oxygen, hydrogen, phosphorus, calcium, and _____
nitrogen
_______ electrons are the electrons found in the outermost shell of the electron cloud.
Valence
Atoms of the same element that differ only in the number of neutrons are known as _____
isotopes
A cation has a net _____ charge.
positive
What is the term for an ion with a net negative charge (more electrons than protons)? Cation Isotope Electron Anion
Anion
Choose the six most abundant (by weight) elements that account for 98.5% of the body weight.
Carbon, oxygen, hydrogen, phosphorus, calcium, and nitrogen
What term refers to a covalent bond in which the electrons are not equally shared?
Polar
If an atom has 2 electrons in its innermost shell and 3 electrons in its outmost shell, how many valence electrons does it have?
3
Salt on a watermelon is an example of a ______.
mixture
Deuterium and tritium are isotopes of hydrogen. What is different about them?
They have a different number of neutrons
What term can be used to describe any molecule that is non-polar and does not dissolve in water?
Hydrophobic
What type of ion has lost an electron and, consequently, has a net positive charge?
Cation
Which term refers to polar molecules that dissolve in water?
Hydrophilic
The chlorine atom gains electrons to become a chloride ______.
anion
