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Science 8 > Chapter 11- Elements and Chemical Bonds > Flashcards

Chapter 11- Elements and Chemical Bonds Flashcards

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1
Q

Valence electron

A

An outermost electron of an atom that participates in chemical bonding

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2
Q

Model that represents valence electrons in an atom as dots around the elements chemical symbol

A

Electron dot diagram

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3
Q

Chemical bond formed when two atoms share one or more pairs of valence electrons

A

Covalent bond

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4
Q

Molecule

A

Group of atoms held together by covalent bonding that acts as an independent unit

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5
Q

Polar molecule

A

Molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons

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6
Q

Group of chemical symbols and numbers that represent the elements and number of atoms each element has that makes up an atom

A

Chemical formula

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7
Q

An atom that is no longer electrically neutral because it has lost or gained valence electrons

A

Ion

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8
Q

Ionic bond

A

The attraction between positively and negatively charged ions in an ionic compound

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9
Q

Bond formed when many metal atoms charged their pooled valence electrons

A

Metallic bond

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10
Q

How can the periodic table help find the number of valence electrons in an element?

A

Groups 1-2, 13-18 show us how many electrons an element has. The group number (ones place) tell us

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11
Q

Why are halogens reactive but not noble gases?

A

Elements want 8 valence electrons, like noble gases

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12
Q

Force that holds two or more atoms together

A

Chemical bond

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13
Q

Characteristics of Ionic Bonds?

A

Solid crystals, high melting and boiling point, dissolve in water, solids are poor conductors of electricity and thermal energy, in water solutions they conduct electricity

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14
Q

Example of an ionic bond

A

Salt (Na+ Cl-)

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15
Q

Characteristics of covalent bonds

A

Gas, liquids or solids, low melting and boiling points, often not able to dissolve in water, poor conductors if thermal energy and electricity, dull appearance

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16
Q

Example of a covalent bond

A

Water (one negative charge with two positives, (H2O)

17
Q

Characteristics of metallic bonds

A

Usually solid at room temperature, high melting and boiling points, do not dissolve in water, good conductors of thermal energy and electricity, shiny surface, hammered into sheets and pulled into wires

18
Q

Example of a metallic bond

A

Aluminium

19
Q

Non metal atoms with non metal atoms

A

Covalent

20
Q

Nonmetal ions with metal ions

A

Ionic

21
Q

Metal ions with metal ions

A

Metallic

22
Q

How is a metallic bond formed?

A

When many metal atoms share their pooled valence electrons (sea of electrons)

23
Q

What is the attraction between positively and negatively charged ions in an ionic compound?

A

Ionic bond

24
Q

How is CO2 arranged?

A

2’atoms of oxygen bounded to one atom of carbon

25
Q

A chemical formula…..

A

Describes the type of atoms in a compound or molecule, but does not explain the shape of appearance of a molecule

26
Q

Shows atoms and valence electrons

A

Electron dot diagram

27
Q

Structural formula

A

Shows atoms and lines, each line represents one shared pair of valence electrons

28
Q

Balls represent atoms and sticks represent bonds

Used to show bond angles

A

Ball and stick model

29
Q

Spheres represent atoms, used to show 3-D arrangement of atoms

A

Space filling model

30
Q

How does atomic number change?

A

It’s increases from left to right as you move across a period

31
Q

What is a row in the periodic called?

A

Period

32
Q

What is a column called?

A

A group

33
Q

What do groups (vertical columns) have in common?

A

Similar chemical properties and react with other elements the same way.
(Melting point, boiling point, 1-2 and 13-18 have the same number of valence)

34
Q

Explain polar molecules

A

It has a partial positive end and a partial negative end due to unequal sharing of valence electrons

35
Q

What happens to an electron in an ionic compound ?

A

Nonmetals gains the electron lost by the metal

36
Q

What is the strongest type of covalent bond?

A

Triple bond

More bonds means it’s stronger

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