Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
22 Cards in this Set
- Front
- Back
|
Binding energy |
The energy required to break the nucleus into protons and neutrons. High BE is stable. |
|
|
Element is defined by which subatomic particle? |
Proton # is the atomic number, Z. changes in neutron create isotopes, chages in proton create a new element. |
|
|
Mass number |
The number of protons + neutrons. This is the atomic weight. example. Hydrogen atom is one AMU because it is only one proton. Technically the atomic weight is the weighted average of all the naturally occurring isotopes. |
|
|
Isotopes |
two or more elements with same number of protons and differing numbers of neutrons. |
|
|
Size trends and gaining/losing atoms |
If you lose an electron, you will become smaller as the effect of the nucleus on each of the remaining electrons will increase.If you gain an electron, you get bigger. General size trend is that size increases down a group and decreases down a period. Francium is big. Lower left. So, Na is way bigger than Cl. But Cl- is bigger than Na. |
|
|
Groups/families vs period. |
periods are rows, groups/families are columns. |
|
|
Common groups |
From left to right. Alkali, alkaline,oxygen group, halogens, noble gases. |
|
|
Metals |
Easily lose electrons to form positive ions and positive oxidation states. SEA of electrons.This allows them to conduct easily, shine, and stretch. They have a loose hold on valence electrons, letting them flow about. |
|
|
alkali metals |
reactive with water. form +1 cations. like sodium. |
|
|
electron affinity |
the willingness of a aotm to accept an additional electron. measured in the energy released upon electron addition. |
|
|
principle quantum number |
Size of shell and energy level of electrons in the shell |
|
|
small atoms are better at forming pi bonds, nitrogen is better than phosphorus. but large atoms can use d orbitals to form extra bonds. |
ya |
|
|
Which elements only have one electorn in the s oribital |
Cr and Cu Cr is [Ar] 4s1 3d5 |
|
|
Plancks and energy transfer |
E=hF |
|
|
paramagnetic vs diamagnetic |
parmagnetic is when elements have unpaired electrons(unfiled subshell). they wull align with an external magnetic field. diamagnetic is when there are no unpaired electrons, so they don't respond to a magnetic field. |
|
|
photoelectric effect |
electrons are jected by one to one photon-electron collisions. the energy of the ejected electron is determined by the frequency, not the intesrity of the light. think planks equation. |
|
|
bond dissociation energy |
the energy required to seperate bond. the higher, the more stable. |
|
|
Breaking a bond. Exothermic or endothermic? |
Endothermic. you need to apply energy to break the bond. The bond increases stability, to go against that means you need to pay some energy |
|
|
hydrogen bond. |
strongest intermolecular force, but they are still weaker than covalent bonds. NOF |
|
|
empirical vs molecular formula |
empirical is smallest whole number ratio of elements. molecular is the exact number of elemental atoms. Glucose- empirical CH2O molecular C6H12O6 |
|
|
percent yield |
actual/theoretical times 100 |
|
|
Radioactive decay types |
Alpha decay- Loss of an alpha particle, which is a helium nucleus. This is a loss of 2 neutrons and 2 protons. Beta minus decay- The breakdown of a neutron into a proton and an electron. The electron is lost. The new element keeps the same mass but increases in atomic number by one. Beta plus decay(positron emission)- A proton becomes a neutron by releasing a positron. the mass number stays the same, but the atomic number goes down by one. electron capture- the element absorbs an electron, turning a proton into a neutron. There is a loss of atomic number. Gamma decay- when an electron and positron combine, mass is annihilated into energy in the form of gamma rays. |
