Chemistry, 9, 9.1

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In moving top to bottom in a column near the right edge of the periodic table, electronegativities tend to (1)_______ and the shielding effect tends to (2)________

(1) = Decrease (b.) (2) = Increase (a.)

In moving from bottom to top in a column near the left edge of the periodic table, electronegativities tend to (1)_________ and the shielding effect tends to (2)__________

(1) = Increase (a.) (2) = Decrease (b.)

In moving from left to right in a row of the periodic table, electronegativities tend to (1)_______ and the shielding effect tends to (2)________

(1) = Increase (a.) (2) = Stay the same (c.)

Malleable

capable of being changed; easily shaped

The ability of a substance to carry an electric current

conductivity (j.)

Ability to be drawn into a thin wire

ductility (c.)

A "sea of electrons"

metallic bond (g.)

Diatomic molecules of elements always have

nonpolar covalent bonds (b.)

Electrons shared unequally between two atoms

polar covalent bond (f.)

A decrease in the attraction exerted by an atomic nucleus on valence electrons

shielding effect (a.)

ΔEN = 3.0

Ionic bond (d.)

ΔEN

The electronegativity difference between two bonding atoms. The EN is an abbreviation for electronegativity and Δ is the Greek letter delta meaning "difference".

Metallic bond

a bond formed by the attraction between positively charged metal ions and the electrons around them

Polar covalent bond

A covalent bond in which electrons are not shared equally

Electrical Conductivity

A measure of how easily electrons can flow through a material to produce an electrical current

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

Ductile

A term used to describe a material that can be pulled out into a long wire.

The valence electrons in a metal

Are shared among all atoms (d.)

𝛿-

Delta minus

𝛿+

Delta plus

In ΔEN, the Greek letter delta (Δ) stands for

Difference (b.)

The measure of an atom's ability to attract electrons in a chemical bond

Electronegativity (I.)

A bond is considered to be ionic if the difference in electronegativities between the two atoms of which it is formed is

Greater than 2.0 (b.)

Ability to be hammered or rolled into a thin sheet

Malleability (h.)

A value of 0.3 for ΔEN of atoms of two elements suggests that the bond between them is

Nonpolar covalent (b.)

ΔEN = 0.3

Nonpolar covalent bond (e.)

Symbolized by 𝛿

Partial charge (b.)

Shielding effect

The reduction of the attractive force between a nucleus and its outer electrons due to the blocking effect of inner electrons

Carbon and bromide

ΔEN = 0.3 Type of bond: Nonpolar covalent

Hydrogen and germanium

ΔEN = 0.3 Type of bond: Nonpolar covalent

Lithium and sulfur

ΔEN = 1.5 Type of bond: Polar covalent

Magnesium and nitrogen

ΔEN = 1.8 Type of bond: Polar covalent

Fluorine and silicon

ΔEN = 2.2 Type of bond: Ionic


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