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Semester 2 Extra Credit Exam Spring 2021

Total questions: 50

Worksheet time: 4hrs 10mins

Name
Class
Date
1.

In a chemical formula, which ion is written first?

a)

heaviest

b)

smallest

c)

anion

d)

cation

2.

The charge on an ionic compound :

a)

is neutral

b)

is positive

c)

is negative

d)

may be positive, negative or neutral

3.

In a chemical formula for a compound, the subscript

a)

is written above the chemical symbol

b)

can be a fraction or a whole number

c)

is written in front of the chemical symbol

d)

tells the number of atoms or ions present

4.

Which of the following elements has two different positive charges?

a)

aluminum

b)

sodium

c)

copper

d)

silver

5.

Cations

a)

have lost electrons, are +

b)

have gained electrons, are neutral

c)

have no electrons

d)

are negative

6.

To form bonds, atoms can do all of the following, except: (More than one answer)

a)

lose electrons

b)

divide electrons

c)

multiply electrons

d)

gain electrons

7.

Which of the following elements would not form any bonds?

a)

W

b)

Ba

c)

Fe

d)

Kr

8.

An Atom will stop bonding when

a)

it loses all of its electrons

b)

it has eight electrons in the outer shell

c)

it shares all of its electrons

d)

it becomes a noble gas

9.

In a crystal, cations and anions are arranged

a)

alphabetically

b)

so all anions are together

c)

by mass

d)

alternately

10.

Polyatomic ions

a)

are a group of atoms with a charge

b)

contain at least three elements

c)

always have a subscript

d)

are mostly made of metals

11.

The charge on a covalently bonded particle is

a)

neutral

b)

positive

c)

negative

d)

may be positive, negative or neutral

12.

Which one of the following elements do not form covalent bonds?

a)

H

b)

At

c)

Se

d)

K

13.

Which one of the following elements forms a diatomic particle?

a)

Si

b)

Na

c)

O

d)

P

14.

If a chemical formula contains a ______ then it must be an ionic compound

a)

metal

b)

subscript

c)

set of parenthesis

d)

non-metal

15.

Covalent bonds form by_________their valence electrons

a)

dividing

b)

losing

c)

sharing

d)

gaining

16.

How many total electrons are shared in a double bond?

a)

1

b)

2

c)

4

d)

8

17.

Which atom would form 3 bonds?

a)

N

b)

Ar

c)

Si

d)

F

18.

Covalent bonds form from:

a)

two or more ions

b)

metals and non-metals

c)

metals only

d)

non-metals

19.

Are solids at room temperature

a)

ionic

b)

covalent

20.

Generally does not dissolve in water:

a)

ionic

b)

covalent

21.

Some are polar

a)

ionic

b)

covalent

22.

Formed from a metal and non-metal

a)

ionic

b)

covalent

23.

Many are non-polar

a)

Ionic

b)

Covalent

24.

tend to be liquids or gases at room temperature

a)

ionic

b)

covalent

25.

also known as salts

a)

ionic

b)

covalent

26.

contain an anion and a cation

a)

ionic

b)

covalent

27.

All are polar

a)

ionic

b)

covalent

28.

thermochemistry studies the changes of _______ in chemical reactions and phase changes.

a)

amounts of substances

b)

ionic and covalent bonds

c)

reaction rates

d)

heat energy

29.

In a camp fire what is the system?

a)

the fire

b)

everything around the fire

30.

In a camp fire the surroundings are :

a)

the camp fire

b)

everything around the fire

31.

If you put an ice cube on your hand and it started to melt, what is happening?

a)

heat is moving from your hand to the ice

b)

your hand is absorbing heat from the ice

c)

heat is condensing into the water

d)

you are perspiring

32.

The Law of Conservation of Energy states that:

a)

energy does not have mass

b)

energy cannot be stored

c)

energy can be transferred

d)

energy cannot be created or destroyed

33.

Heat travels

a)

from hot to cold

b)

from down to up

c)

forward to reverse

d)

from cold to hot

34.

All of the following are units of heat, except

a)

calorie

b)

kilocalorie

c)

degree celsius

d)

joule

35.

Heat is which type of energy?

a)

electrical

b)

kinetic

c)

light

d)

potential

36.

Note the following equation:

CH4 + 3O2 --> 2CO2 + 2H2O + 2000kJ

This reaction is

a)

exothermic

b)

endothermic

c)

isothermic

d)

parathermic

37.

All of the following are characteristics of an endothermic reaction, except...

a)

feels colder

b)

temp decreases

c)

system absorbs heat

d)

an explosion

38.

Direction of heat flow is always based on the

a)

universe

b)

surroundings

c)

system

d)

container

39.

If heat is (-) the reaction is:

a)

exothermic

b)

endothermic

c)

completed

d)

unstable

40.

If heat is (+) the reaction is

a)

exothermic

b)

endothermic

c)

completed

d)

unstable

41.

The common substance that has a high specific heat is

a)

water

b)

lead

c)

concrete

d)

sand

42.

Ca

a)

Halogen

b)

Transition Metal

c)

Alkali Metal

d)

Alkaline Earth Metal

43.

Si

a)

Metalloid

b)

Transition Metal

c)

Noble Gas

d)

Alkali Metal

44.

Ar

a)

Metalloiid

b)

Noble Gas

c)

Transition Metal

d)

Halogen

45.

F

a)

Noble Gas

b)

Alkali Metal

c)

Metalloid

d)

Halogen

46.

Most of the elements in the Periodic Table are

a)

Non-Metals

b)

Gases

c)

Metals

d)

Metalloids

47.

In the Periodic Table, elements are placed in increasing order by:

a)

Valence Number

b)

Atomic Mass

c)

Density

d)

Atomic Number

48.

The Periodic Table was first developed by

a)

Valence Number

b)

Atomic Mass

c)

Mendeleev

d)

Mosley

49.

Which element is in Period 7, Group 5

a)

Bi

b)

Mg

c)

Db

d)

Tc

50.

Elements in a column are called a(an)

a)

period

b)

group

c)

section

d)

grumpy

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