Electron Arrangment Flashcards
1
Q
Ionic bond
A
- electrostatic attraction between oppositely charged ions
2
Q
Types of orbitals
A
S= 1
P= 3
d= 5
F= 7
3
Q
Why are blocks named like that
A
- highest energy occupied she’ll
4
Q
Characteristics of ionic compound
A
- brittle
- solid insulator
- high melting and boiling point
- mainly soluble
5
Q
Giant ionic structures
A
- giant layers of positive and negative ions held by strong electrostatic bonds
- carries moving charge; electrical conductor as solid
- brittle lattices; disruption causing repulsion in structure
6
Q
Dative bonds
A
- shared pair of electrons from same Aton
7
Q
Tetrahedral angles
A
- 109.5
8
Q
Trigonal planar angle
A
- 120
9
Q
Bent angle (1LP)
A
- 118
10
Q
Trigonal pyramid angle
A
- 107
11
Q
Bent angle (2LP)
A
-104.5
12
Q
Trigonal bipyramid angles
A
- 90
- 120
13
Q
Octahedral angles
A
90
14
Q
Square planar angles
A
-90
15
Q
Electronegativity
A
- ability for atom to attract a bonded pair of electrons in covalent bond
- increase with less protons and electron shells
16
Q
London forces
A
- in all molecules
- when electrons move towards positive charge in atoms
- instantaneous
- more electrons = stronger attractive five
17
Q
Orbital
A
- where electrons reside in and holds up to 2 with opposite spins
18
Q
How many electrons in an orbital
A
2
19
Q
How many electrons in a shell?
A
2(n squared)
