Quiz 1 Chap 2&3 Flashcards
Atoms, Bonds, and Water, and Biological Molecules
primordial soup
water in oceans many years ago, where life originated
matter
made up of elements, containing mass
elements
substance that cannot be broken down to other substances by chemical reactions
compounds
substance consisting of 2 or more elements in a fixed ratio
- different from the individual elements in its characteristics
how many elements are essential to life? which elements are essential to life?
25 elements total, although some are trace elements (minute quantities)
- 96% of human body. weight is oxygen, carbon, hydrogen, and nitrogen
- then calcium, phosphorus, potassium, and sulfur
atom
smallest unit of an element
composed of subatomic particles (protons, neutrons, electrons)
electrons move around nucleus in orbitals
what does the chemical behavior of an element depend on?
the number of UNPAIRED valence elections in the valence shell
molecule
atoms that stay close together by chemical bonds (can be 2 of the same atom)
intramolecular forces
bonds that hold molecules together (ionic bonds, covalent bonds, polar covalent bonds)
intermolecular forces
bonds that hold different molecules together (hydrogen bonds, Van der Waal bonds)
bonding capacity of an element
of covalent bonds that each element can form (# of unpaired electrons in the valence shell)
ionic bonds
- give away or steal an electron
- formed by attraction of two oppositely-charged ions
- strong in dry environment
- weak in aqueous environment (water is polar, it splits apart ions)
- formed by a metal and a non-metal
salts
compounds formed by ionic bonds, typically crystals containing huge numbers of cations and anions
covalent bonds
- share valence electrons so that both atoms can fill their valence shells
- can from between atoms of the same or different elements
- very strong bonds
- bonds made and broken from chemical reactions
nonpolar covalent bonds
no charges on molecule, atoms share electron(s) equally
polar covalent bonds
partial positive and negative charges on each molecule due to the electron not being shared equally (one atom is more electronegative)
hydrogen bonds
result of attraction between a partially positive hydrogen (covalently bonded to a more electronegative atom like oxygen) and another electronegative atom
- what causes water to adhere to itself
- hydrogen typically bonded to oxygen or nitrogen in living cells
- weak individually, but many can be strong
role of hydrogen bonds in biological systems
- bonds between nitrogenous bases in DNA, able to be unzipped
- factor in protein structure
why do substances dissolve in water??
water is the universal solvent because of its polarity (oxygen has partial negative, hydrogens have partial positive)
- ionic bonds broken as ions are attracted to these partial charges
- large proteins have polar regions on their surfaces which attract water molecules
hydration
ionic bonds break and ions attach/come close to polar water molecules
Van der Waals bond
- intermolecular force
- electrons accumulate randomly in nonpolar molecules (temporary and by chance)
- individually weak, powerful if occurring simultaneously
which type of bond is strongest?
covalent bonds
role of weak bonds (ionic, hydrogen)
- reinforce shape of large molecules
- help molecules adhere to each other
what determines molecular shape?
the position of valence orbitals
- orbitals may hybridize in covalent bonds
what is the importance of molecular shape?
biological molecules recognize and interact with each other based on shape, so molecules with similar shape can have similar biological effects
- i.e. morphine and endorphins
significance of water in organisms
most cells surrounded by water and are made up of 70-95% water
what 4 properties of water facilitate life processes
- cohesive behavior
- ability to moderate temperature
- expansion upon freezing
- versatility as a solvent
cohesion
hydrogen bonds hold water molecules together
- causes surface tension
- helps transport of water against gravity in plants
adhesion
attraction between water and other substances
- notably, plant cell walls (again allows for transport up plants)
what is the significance of water’s high specific heat capacity?
- can absorb/release large amounts of heat without changing its own temperature much, which helps maintain HOMEOSTASIS
- **heat is absorbed when hydrogen bonds break (ice crystals breaking) and released when bonds form
why does water expand when it freezes?
hydrogen bonds are more ordered, causing molecules to be farther apart (less dense)
at what temp is water the most dense?
4 celsius