9th Grade Chapter 7 Kms Flashcards Preview

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Flashcards in 9th Grade Chapter 7 Kms Deck (20)
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1
Q

difference between a molecule and compound?

A

A molecule is 2 or more atoms joined together

A compound is 2 or more elements joined together to make a new substance

2
Q

Explain what a mixture is and the 2 types

A

A mixture (not pure) is 2 or more compounds mixed together but not chemically combine (salt and sand can be mixed but separated once you add water)

  1. Homogeneous- evenly mixed, same physical property throughout
  2. Heterogeneous- unevenly mixed
3
Q

How to tell if it’s a mixture, what can you use to seperate?

A

Color, boiling and melting point, state, luster

4
Q

Solvent?

A

Does the dissolving

5
Q

Solute?

A

Gets dissolved

6
Q

Soluble/insoluble are also called

A

Missable and inmissable

7
Q

Explain collide suspension

A

It’s when somehing is insoluble but particles are suspended by brownish motion (in between state before dissolving)

8
Q

What’re the 3 types of compounds/bonds

A

Ionic, covalent, and metallic

9
Q

Explain ionic bond and ions

A

Electrical attraction between positive and negative atoms (ion) and no sharing of electrons
Fairly weak
When an atom is charged Na to Na+ (losing or gaining an electron causing an atom to have a charge)

10
Q

Give an example of an ionic bond

A

Salt crystals made of Na+ and Cl-

11
Q

Explain covalent bonds

A

Electrical attraction between atoms due to the sharing of 2 or more electrons
Strong bond (10 times stronger than ionic)
Not good conductors
H H < between each H and the O is 2 electrons
o being shard

12
Q

Explain metallic bonds

A

Like covalent bonds but shared electrons can travel anywhere they’d like (electron sea/delocalized)
Good conductors of heat/electricity

13
Q

Explain the difference between polar and nonpolar covalent bonds

A

Polar- electrical bonds (positive and negative ends)

Non polar- electrical symmetry (no positive/negative ends)

14
Q

Empirical formula,

A

Simplest ratio of atoms in a molecule

C6H12 to CH2

15
Q

3 intermolecular forces?

A

Dipole dipole
London
Hydrogen

16
Q

Explain the dipole dipole force

A

Between 2 polar molecules, relatively strong
H H o
O. H H

17
Q

Explain the London force

A

Instantaneous dipole
Stop time and both electrons theatre being shared might for a split second be in the middle causing the balance to be off and causing a partial positive side
Very weak

18
Q

Explain the hydrogen bond

A

Only when hydrogen bonds to oxygen, fluorine, nitrogen
VERY strong
Exposed hydrogen proton (bc there’s only 1) and has atoms attracted to it’s positiveness

19
Q

What’re the effects of the intermolecular forces

A

Melting point, boiling point, vapor pressure, solubility

20
Q

The simplest expression of any atom is ?

A

That element