Chapter 6 - Claire Flashcards
What Δ EN values create an ionic bond?
1.7 to 3.3
What Δ EN values create a covalent bond?
0 to 1.7
Where is atomic radius the largest?
Bottom left of the periodic table
Are cations smaller or larger than the neutral atom?
Smaller
Are anions smaller or larger than the neutral atom?
Larger
Def. the net positive charge experienced by an electron in a multi electron atom, representing less than the full nuclear charge as inner electrons repel outer electrons, offsetting some of the nucleus’s inward pull(I.e. shielding effect)
Effective nuclear charge
Def. the repulsive action of inner core electrons in outer valence electrons, effectively reducing the nucleus’s inward pull, causing the atom to increase in size
Shielding effect
Coulomb’s law states that the _______ of force depends directly on the amount of ____________
Strength, electrostatic charge
Which two elements have no shielding effect?
Hydrogen and helium
What are the four types of charge?
- Proton-proton repulsion
- Neutron-proton attraction (residual strong force)
- Electron-electron repulsion
- Nucleus-electron attraction
Def. an expression of the size of an atom, representing the typical distance from the center of its nucleus to the boundary of its electron cloud
Atomic radius
Def. an estimate of the size of an atom, based on half the distance between covalently bonded atoms
Covalent radius
Def. an estimate of an the size of a metal atom based on half the distance between the nuclei of adjacent atoms in a metal lattice
Metallic radius
What affects an electron cloud/ an atoms size?
- Number of occupied shells
2. Amount and type of charge
Def. predictable and regular patterns of cyclical change in elemental properties throughout the periodic table, moving either vertically or horizontally
Periodic trends
Def. the amount of energy required to remove the most loosely held electron from a gaseous atom to form a cation, or from a cation to increase its positive charge
Ionization energy
Where are electrons held the most loosely?
Bottom right of the periodic table
Def. a chemical property that describes an atom’s (or a group of atoms’) ability to attract electrons towards itself
Electronegativity
Def. the change in energy when an atom gains an electron to form an anion, or when an anion gains another electron, increasing its negative charge
Electron affinity
The higher the electronegativity, the higher the ____________
Electron affinity
def. A numerical value representing the difference in the electronegativities of two atoms
ΔEN
def. A covalent bond between non-metal atoms with the same electronegativities, where
electron sharing is equal between them
Nonpolar covalent bond
Are electrons ever transferred to a different atom?
No, they only effectively transfer because there is always some sort of electronegativity
def. A covalent bond between two non-metal atoms in which electron sharing is sufficiently
unequal that the bond displays significant and meaningful ionic nature
Polar covalent bond
Where is the electron sharing is equal or nearly equal between the atoms and the
bond has predominantly covalent character with little to no ionic character?
Nonpolar bonds
Where is the electron sharing is disproportionately uneven enough that the bond has
predominantly ionic character, with very little covalent character?
ionic bonds
def. The non-integer charge values at the ends of a polar covalent bond, due to the uneven
distribution of electron density within the bond
Partial ionic charges (δ+, δ–)
Where is the electron sharing is uneven enough that
the covalent bond has some ionic nature – more than a nonpolar bond, but less than an ionic?
polar bonds