Unit 1 Flashcards
1
Q
- Atomic size (radius)
A
- as you move down each group, the size of an atom increases because you are adding more orbits or shells
- as you move across a period from left to right, the size of an atom decreases because the positive charge on the nucleus increases causing a greater pull on the widely spaced valance electrons
2
Q
- Ionization energy (IE)
A
- the energy required to remove an electron from an atom
- atoms that give up electrons easily have low IEs
- alkali metals have the lowest IEs of all the groups
- noble gases have the highest IEs
- as you move down a group, electrons in the outer energy levels are further form positive nucleus and therefore easier to remove
3
Q
- Electronegativity
A
- an indicator of the relative ability of an atom to attract shared electrons
- the positively charged nucleus of a small atom like Fluorine can get much closer to the electrons of another atom, more so than a large atom like cesium
- directly correlated to atomic size
4
Q
- Electron affinity
A
- the energy absorbed or released when an electron is added (anion) to a neutral atom
- if energy is needed to add an electron, the resulting anion will be unstable and will soon lose the electron
- if energy is released (made more stable) when an electron is added, the resulting anion will be stable
- EA tends to decrease down a group and increase as you move across a period from left to right
5
Q
Periodic law
A
the chemical and physical properties of the elements repeat in a regular pattern when they are arranged according to atomic #
6
Q
Groups/columns
A
vertical
7
Q
Periods/rows
A
horizontal
8
Q
What is atom?
A
- smallest particle of an element that still retains the identity and properties of the element
- about 10^-10 m in diameter
- made up of subatomic particles
9
Q
atomic mass unit (u)
A
- protons and neutrons each have a mass of 1u
- electrons have too small a mass to be acknowledged
10
Q
X
A
atomic symbol
11
Q
A
A
atomic mass (# of protons + # of neutrons)
12
Q
Z
A
atomic # (# of protons)
13
Q
isotopes
A
atoms of an element that have the same # of protons but diff # of neutrons; similar chem properties just diff mass
14
Q
radioisotopes
A
unstable isotopes, their nuclei decay releasing subatomic particles
15
Q
modern atomic theory
A
- All matter is made up of tiny particles called atoms. Each atom is made up of smaller subatomic particles (e, p, n).
- The atoms of 1 element can’t be converted into the atoms of any other element by a chemical reaction.
- Atoms of 1 element have the same properties, such as average mass and size. These properties are different from the properties of the atom of any other element.
- Atoms of different elements combine in specific proportions to form compounds.